WARNING: THIS WEBSITE DEFIES THE SECOND LAW OF … · Web viewTwo trials for the reaction above are carried out, and the heat flow is measured using a calorimeter. In the first trial,

2016 test AP Questions remade correct answers are bolded

Based on # 1

1) Which of the following liquids experiences dipole-dipole intermolecular forces?a) O2(l) b) CCl4(l) c) SO3(l) d) CF2Cl2

2) Which of the following liquids experiences dipole-dipole intermolecular forces?a) F2(l)b) CF4(l) c) SO3(l) d) CF2Cl2

3) Which of the following liquids experiences dipole-dipole intermolecular forces?a) H2(l) b) CF4(l) c) SO2(l) d) CCl4

Based on # 2:

1) Which of the following best explains why temperature increases cause reaction rates to increase. a) As temperature increases, activation energy increasesb) As temperature increases, activation energy decreasesc) As temperature increases, collisions between reactant particles increasesd) As temperature increases, more collisions between particles have a required amount of energy.

2) Which of the following best explains why temperature increases cause reaction rates to increase. a) As temperature increases, activation energy increasesb) As temperature increases, collisions between particles decreasesc) As temperature increases, particles have more energy, allowing collisions to form productsd) As temperature increases, particles have more energy, and collide less often

Based on # 3

1) A sample of a solid substance conducts electricity in both the solid and liquid phase. Which of the following types of interactions is most likely found between particles in the substance?a) ionic bonds b) metallic bonds c) covalent bonds d) hydrogen bonds

2) A sample of a solid substance conducts electricity in the liquid phase but not the solid phase. Which of the following types of interactions is most likely found between particles in the substance?a) ionic bonds b) metallic bonds c) covalent bonds d) hydrogen bonds

3) A sample of a solid substance does not conduct electricity in either the solid or liquid phase. The solid is not soluble in water. Which of the following types of interactions is most likely found between particles in the pure substance?a) ionic bonds b) metallic bonds c) covalent bonds d) hydrogen bonds

4) A sample of a solid substance does not conduct electricity in either the solid or liquid phase. The solid is soluble in water. Which of the following types of interactions is most likely found between particles in the pure substance? a) ionic bonds b) metallic bonds c) network covalent bonds d) dipole-dipole forces

Based on # 4

N2(g) + 3 H2(g) 2 NH3(g) H<0

1) Gaseous ammonia was synthesized in the presence of a catalyst and allowed to reach equilibrium. Which of the following changes would cause more ammonia to be present in the mixture when equilibrium is reestablished? a) increase the temperature b) increase the container’s volumec) add a chemical that reacts with hydrogen gasd) add hydrogen gas to the container

2) Gaseous ammonia was synthesized in the presence of a catalyst and allowed to reach equilibrium. Which of the following changes would cause more ammonia to be present in the mixture when equilibrium is reestablished? a) decrease the temperature b) increase the container’s volumec) add a chemical that reacts with hydrogen gasd) break up the catalyst into smaller particles

3) Gaseous ammonia was synthesized in the presence of a catalyst and allowed to reach equilibrium. Which of the following changes would cause more ammonia to be present in the mixture when equilibrium is reestablished? a) increase the temperature b) decrease the container’s volumec) add a chemical that reacts with hydrogen gasd) remove nitrogen gas from the container

4) Gaseous ammonia was synthesized in the presence of a catalyst and allowed to reach equilibrium. Which of the following changes would cause more ammonia to be present in the mixture when equilibrium is reestablished? a) decrease the temperature b) increase the container’s volumec) add a chemical that reacts with hydrogen gasd) remove nitrogen gas from the container

Based on # 5

1) Which of the following shows the molecules F2, Cl2, and Br2 in order of their bond enthalpies from least to greatest?a) F2 < Cl2 < Br2

b) Cl2 < Br2 < F2

c) Br2 < Cl2 < F2

d) Br2 < F2 < Cl2

2) Which of the following shows the molecules F2, N2, and Br2 in order of their bond enthalpies from least to greatest?a) F2 < N2 < Br2

b) N2 < Br2 < F2

c) Br2 < F2 < N2

d) F2 < Br2 < N2

3) Which of the following shows the molecules F2, O2, and Br2 in order of their bond enthalpies from least to greatest?a) F2 < O2 < Br2

b) O2 < Br2 < F2

c) Br2 < F2 < O2

d) F2 < Br2 < O2

Based on # 6

Ion Ionic radius (pm)Hg2+ 102Ba2+ 135Al3+ 54Mg2+ 72

1) Based on Coulomb’s Law and the data in the table above, which of the following would have the weakest interactions with an adjacent water molecule in an aqueous solution? a) Hg2+ b) Ba2+ c) Al3+ d) Mg2+

Ion Ionic radius (pm)Hg2+ 102Ba2+ 135Al3+ 54Mg2+ 722) Based on Coulomb’s Law and the data in the table above, which of the following would have the strongest interactions with an adjacent water molecule in an aqueous solution? a) Hg2+ b) Ba2+ c) Al3+ d) Mg2+

Ion Ionic radius (pm)Mg2+ 72Ca2+ 100Al3+ 54K+ 1383) Based on Coulomb’s Law and the data in the table above, which of the following would have the strongest interactions with an adjacent water molecule in an aqueous solution? a) Mg2+ b) Ca2+ c) Al3+ d) K1+

Ion Ionic radius (pm)Mg2+ 72Ca2+ 100Al3+ 54K+ 1384) Based on Coulomb’s Law and the data in the table above, which of the following would have the weakest interactions with an adjacent water molecule in an aqueous solution? a) Mg2+ b) Ca2+ c) Al3+ d) K1+

Based on # 7

Element

electronegativity

Li 0.98

Be 1.57

B 2.04

C 2.55

N 3.04

O 3.44

F 3.98

1) On the basis of the data in the table above, which of the following arranges the bonds in molecules from least to most polar?a) NF3 < NO2 < CF4 < OF2

b) CF4 < NO2 < OF2 < NF3

c) NO2 < OF2 < NF3 < CF4

d) NF3 < NO2 < OF2 < CF4

Based on # 8

X(g) X+(g) + e- IE1 = 580 kJ/molX+(g) X2+(g) + e- IE2 = 1820 kJ/molX2+(g) X3+(g) + e- IE3 = 2750 kJ/molX3+(g) X4+(g) + e- IE4 = 11,600 kJ/mol

For element X, which of the following most likely explains the large difference between the 3rd and 4th ionization energies?a) The effective nuclear charge decreases with each successive ionization energyb) The distance between the nucleus and the electron being removed increases with each successive ionization energyc) The electron removed for the 4th ionization energy has much less energy than the electron removed for the 3rd ionization energyd) The ionic radius increases with each successive ionization energy

Based on # 9

A student performs an acid base titration. The data are plotted above. Which of the following best describes the type of titration done?a) a strong acid was titrated with a strong baseb) a weak acid was titrated with a strong basec) a strong acid was titrated with a weak based) a weak acid was titrated with a weak base

A student performs an acid base titration. The data are plotted above. Which of the following best describes the type of titration done?a) a strong acid was titrated with a strong baseb) a weak acid was titrated with a strong basec) a strong acid was titrated with a weak based) a weak acid was titrated with a weak base

Volume base added

Volume base added

A student performs an acid base titration. The data are plotted above. Which of the following best describes the type of titration done?a) a strong base was titrated with a strong acidb) a weak base was titrated with a strong acidc) a strong base was titrated with a weak acidd) a weak base was titrated with a weak acid

A student performs an acid base titration. The data are plotted above. Which of the following best describes the type of titration done?a) a strong base was titrated with a strong acidb) a weak base was titrated with a strong acidc) a strong base was titrated with a weak acidd) a weak base was titrated with a weak acid

Based on # 11

1) A sample of a compound contains 24.0 g C, 5.0 g H, and 8.0 g O. Which of the following is the empirical formula of the compound? a) C2H5Ob) C4H10Oc) C6H15O2

d) C8H20O2


d) C6H12O2


d) C6H8O2

Based on # 12Compound KspPbBr2 7 x 10-6

CuBr 6 x 10-9

AgBr 4 x 10-13

HgBr2 6 x 10-20

1) The Ksp values of several salts are shown in the table above. A saturated solution of which of the following compounds has the highest Br- concentration?a) PbBr2

b) CuBrc) AgBrd) HgBr2

Compound KspPbI2 1 x 10-10

CuI 1 x 10-12

BiI 8 x 10-19

HgI2 3 x 10-29

2) The Ksp values of several salts are shown in the table above. A saturated solution of which of the following compounds has the highest I- concentration?a) PbI2

b) CuIc) BiId) HgI2

Compound KspPbBr2 7 x 10-6

CuBr 6 x 10-9

AgBr 4 x 10-13

HgBr2 6 x 10-20

1) The Ksp values of several salts are shown in the table above. A saturated solution of which of the following compounds has the lowest Br- concentration?a) PbBr2

b) CuBrc) AgBr

d) HgBr2

Compound KspPbI2 1 x 10-10

CuI 1 x 10-12

BiI 8 x 10-19

HgI2 3 x 10-29

2) The Ksp values of several salts are shown in the table above. A saturated solution of which of the following compounds has the lowest I- concentration?a) PbI2

b) CuIc) BiId) HgI2

Compound KspFeS 8 x 10-19

Tl2S 6 x 10-22

CuS 8 x 10-37

Ag2S 8 x 10-51

2) The Ksp values of several salts are shown in the table above. A saturated solution of which of the following compounds has the lowest S2- concentration?a) FeSb) Tl2Sc) CuSd) Ag2S

Compound KspFeS 8 x 10-19

Tl2S 6 x 10-22

CuS 8 x 10-37

Ag2S 8 x 10-51

2) The Ksp values of several salts are shown in the table above. A saturated solution of which of the following compounds has the highest S2- concentration?a) FeSb) Tl2Sc) CuSd) Ag2S

Compound KspCaCO3 3 x 10-9

CdCO3 1 x 10-12

Ag2CO3 8 x 10-12

Nd2(CO3)3 1 x 10-33

2) The Ksp values of several salts are shown in the table above. A saturated solution of which of the following compounds has the highest CO3

2- concentration?a) CaCO3

b) CdCO3

c) Ag2CO3

d) Nd2(CO3)3

Compound KspCaCO3 3 x 10-9

Ag2CO3 8 x 10-12

PbCO3 7 x 10-14

Y2(CO3)3 1 x 10-31

2) The Ksp values of several salts are shown in the table above. A saturated solution of which of the following compounds has the lowest CO3

2- concentration?a) CaCO3

b) Ag2CO3

c) PbCO3

d) Y2(CO3)3

Based on #s 14 and 15

The following two questions are based on the following information

3 Pb + 2 Au3+ 3 Pb2+ + 2 Au Eo = 1.63 V

Pb2+ + 2e- Pb Eo = ?

Au3+ + 3 e- 2 Au Eo = 1.50 V

1) What is the standard reduction potential for the lead (II) half reaction?a) -3.13 Vb) -0.13 Vc) +0.13 Vd) +3.13 V

2) Which of the following is true for the reaction overall balanced reaction listed above under standard conditions?a) K>1, Go<0b) K>1, Go>0c) K<1, Go>0d) K<1, Go<0

Ni + Cu2+ Ni2+ + Cu Eo = 0.60 V

Ni2+ + 2e- Ni Eo = ?

Cu2+ + 2 e- 2 Cu Eo = 0.34

1) What is the standard reduction potential for the nickel (II) half reaction?a) -0.94 Vb) -0.26 Vc) +0.26 Vd) +0.94 V


Zn + 2 Ag+ Zn2+ + Ag Eo = 1.56 V

Zn2+ + 2e- Zn Eo = ?

Ag+ + e- Ag Eo = 0.80

1) What is the standard reduction potential for the silver ion half reaction?a) -2.36 Vb) -0.76 Vc) +0.76 Vd) +2.36 V


Based on #16

C2H2(g) + H2(g) C2H4(g)For the reaction above, which of the following will most likely increase the rate of reaction?a) decrease the temperature of the reaction containerb) decrease the volume of the reaction containerc) pressurize the system with an inert gas, keeping temperature constantd) remove acetylene (C2H2) from the reaction container

C2H2(g) + H2(g) C2H4(g)For the reaction above, which of the following will most likely increase the rate of reaction?a) decrease the temperature of the reaction containerb) increase the volume of the reaction containerc) pressurize the reaction container with an inert gas, keeping temperature constantd) add a heterogeneous catalyst to the reaction container

C2H2(g) + H2(g) C2H4(g)For the reaction above, which of the following will most likely increase the rate of reaction?a) increase the temperature of the reaction containerb) increase the volume of the reaction containerc) pressurize the reaction container with an inert gas, keeping temperature constantd) remove acetylene (C2H2) from the reaction container

Based on # 17

Which of the following molecules is least soluble in water?a) CH2F2 b) CH3OH c) CH2O d) CH3CH3

Which of the following molecules is least soluble in water?a) CF3Cl b) CH3OH c) CH2O d) CF4

Which of the following molecules is least soluble in water?a) CH3OH b) CH3 CH2OH c) CH3CH3CH2OH d) CH3CH3CH3CH2OH

Based on # 18

At room temperature, bromine, Br2, is a liquid. Which of the following provides a characteristic of bromine with a correct explanation?a) bromine has a higher boiling point than chlorine (which is a gas at room temperature) because bromine has more electrons than chlorineb) bromine has a lower first ionization energy than krypton (an atomic element that is a gas at room temperature) because bromine is a liquid at room temperature.c) bromine is a not a good conductor of electricity because it has lone pairs of electrons.d) bromine is soluble in water because bromine is polar.

At room temperature, iodine, I2, is a solid. Which of the following provides a characteristic of iodine with a correct explanation?a) iodine has a higher melting point than bromine (which is a liquid at room temperature) because iodine has more electrons than bromineb) iodine has a lower first ionization energy than xenon (an atomic element that is a gas at room temperature) because iodine is a solid at room temperature.c) iodine is a not a good conductor of electricity because it has lone pairs of electrons.d) iodine is soluble in water because iodine is polar.

At room temperature, chlorine, Cl2, is a gas. Which of the following provides a characteristic of chlorine with a correct explanation?a) chlorine has a lower boiling point than bromine (which is a liquid at room temperature) because chlorine has fewer electrons than bromineb) chlorine has a lower first ionization energy than argon (an atomic element that is also a gas at room temperature) because elemental chlorine forms molecules whereas elemental argon does not.c) chlorine is a not a good conductor of electricity because it has lone pairs of electrons.d) chlorine is soluble in water because chlorine is polar.

Based on # 19Substance Boiling Point (oC)CBr4(l) 190CCl4(l) 77Based on the information in the table above, which liquid has a higher vapor pressure at 25oC and why?a) CBr4(l), because it has weaker intermolecular forcesb) CBr4(l), because it has stronger intermolecular forcesc) CCl4(l), because it has weaker intermolecular forcesd) CCl4(l), because it has stronger intermolecular forcesSubstance Boiling Point (oC)

CBr4(l) 190CHBr3(l) 150

Based on the information in the table above, which liquid has a higher vapor pressure at 25oC and why?a) CBr4(l), because it has weaker intermolecular forcesb) CBr4(l), because it has stronger intermolecular forcesc) CHBr3(l), because it has weaker intermolecular forcesd) CHBr3(l), because it has stronger intermolecular forces

Substance Boiling Point (oC)CBr4(l) 190CCl4(l) 77Based on the information in the table above, which liquid has a lower vapor pressure at 25oC and why?a) CBr4(l), because it has weaker intermolecular forcesb) CBr4(l), because it has stronger intermolecular forcesc) CCl4(l), because it has weaker intermolecular forcesd) CCl4(l), because it has stronger intermolecular forces

Substance Boiling Point (oC)CBr4(l) 190CHBr3(l) 150

Based on the information in the table above, which liquid has a lower vapor pressure at 25oC and why?a) CBr4(l), because it has weaker intermolecular forcesb) CBr4(l), because it has stronger intermolecular forcesc) CHBr3(l), because it has weaker intermolecular forcesd) CHBr3(l), because it has stronger intermolecular forces

Based on #20

HX(aq) + Y-(aq) HY(aq) + X-(aq) K = 1.5 x 10-5

Based on the information above, which is the strongest acid?a) HX(aq) b) Y-(aq) c) HY(aq) d) X-(aq)


Based on the information above, which is the weakest acid?a) HX(aq) b) Y-(aq) c) HY(aq) d) X-(aq)

HX(aq) + Y-(aq) HY(aq) + X-(aq) K = 1.5 x 105

Based on the information above, which is the weakest acid?a) HX(aq) b) Y-(aq) c) HY(aq) d) X-(aq)


Based on the information above, which is the strongest acid?a) HX(aq) b) Y-(aq) c) HY(aq) d) X-(aq)


Based on the information above, which is the strongest base?a) HX(aq) b) Y-(aq) c) HY(aq) d) X-(aq)


Based on the information above, which is the weakest base?a) HX(aq) b) Y-(aq) c) HY(aq) d) X-(aq)


Based on the information above, which is the weakest base?a) HX(aq) b) Y-(aq) c) HY(aq) d) X-(aq)


Based on the information above, which is the strongest base?a) HX(aq) b) Y-(aq) c) HY(aq) d) X-(aq)

Based on #21

Pb(NO3)2(aq) + Na2CO3(aq) PbCO3(s) + Na2CO3(aq)

A student wanted to determine the molarity of lead(II) nitrate in a solution. She added a large excess of sodium carbonate solution to a sample of the Pb(NO3)2 solution. The lead(II)carbonate precipitate was collected via filtration and dried. After analyzing the data, the student results suggested the lead(II) nitrate concentration was 3% higher than expected. Which of the following could account for this error?a) The precipitate was dried at too high a temperature, causing some of the solid to decompose into CO2 and PbO. b) The filter paper allowed some of the precipitate to escape into the liquid portionc) Not all the liquid and precipitate was transferred to the filter paperd) the precipitate was not rinsed with distilled water after collection


A student wanted to determine the molarity of lead(II) nitrate in a solution. She added a large excess of sodium carbonate solution to a sample of the Pb(NO3)2 solution. The lead(II)carbonate precipitate was collected via filtration and dried. After analyzing the data, the student results suggested the lead(II) nitrate concentration was 3% lower than expected. Which of the following could account for this error?a) The precipitate was not dried completely b) The filter paper allowed some of the precipitate to escape into the liquid portionc) The student spilled a very small amount of the sodium carbonate solution before adding it to the lead(II) nitrate solutiond) the precipitate was not rinsed with distilled water after collection


A student wanted to determine the molarity of lead(II) nitrate in a solution. She added a large excess of sodium carbonate solution to a sample of the Pb(NO3)2 solution. The lead(II)carbonate precipitate was collected via filtration and dried. After analyzing the data, the student results suggested the lead(II) nitrate concentration was 3% higher than expected. Which of the following could account for this error?a) The precipitate was not dried completely b) The filter paper allowed some of the precipitate to escape into the liquid portionc) The student spilled a small amount of the sodium carbonate solution before adding it to the lead(II) nitrate solutiond) the precipitate was rinsed many times with distilled water after collection

Based on #22, 23

A student titrated a 30.0 mL sample of hydrochloric acid with 1.00 M NaOH. She plotted the experimental data and obtained the graph above.

1) At point B in the plot, which ions have a concentration greater than 0.10 M?a) only Na+, Cl-

b) only Na+, Cl-, OH-

c) only Na+, Cl-, H+

d) only Na+, Cl-, H+, OH-

2) How would the titration curve above differ if the student used 0.100 M NaOH rather than 1.00 M NaOH for the titrant?a) The initial pH would be 1, rather than 0b) The pH at equivalence would be higher than in the original titrationc) The pH well past the equivalence point would be lower than in the original titrationd) The pH well past the equivalence point would be higher than in the original titration

(following are questions not on the exam – but added by Edye)

3) If the student accidentally spilled some of the HCl after measuring out 30.0 mL and before using it for the titration, what could be the most likely true[HCl]?a) 2.00 M HCl b) 1.98 M HCl c) 2.02 M HCl d) 0.49 M HCl

A student titrated a 30.0 mL sample of hydrochloric acid with 0.500 M NaOH. She plotted the experimental data and obtained the graph above.

1) At point B in the plot, which ions have a concentration greater than 0.10 M?a) only Na+, Cl-

b) only Na+, Cl-, OH-

c) only Na+, Cl-, H+

d) only Na+, Cl-, H+, OH-


(following are questions not on the exam – but added by Edye)

3) If the student accidentally spilled some of the HCl after measuring out 30.0 mL and before using it for the titration, what could be the most likely true[HCl]?a) 1.00 M HCl b) 1.01 M HCl c) 0.99 M HCl d) 0.49 M HCl

A student titrated a 10.0 mL sample of a monoprotic acid, HX, with 0.500 M NaOH. She plotted the experimental data and obtained the graph above.

1) At point D in the plot, which ions have a concentration greater than 0.10 M?a) only Na+

b) only Na+, X-

c) only Na+, X-, H+

AB

C

D

d) only Na+, X-, OH-


(following are questions not on the 2016 exam – but added by Edye)

3) If the student accidentally spilled some of the HX solution after measuring out 10.0 mL and before using it for the titration, what could be the most likely true[HX]?a) 1.00 M HCl b) 1.01 M HCl c) 0.99 M HCl d) 0.49 M HCl

3) If the student rinsed the buret with water immediately before adding the titrant to the buret and then starting the titration what could be the most likely true[HX]?a) 1.00 M HCl b) 1.01 M HCl c) 0.99 M HCl d) 0.49 M HCl

4) What is the pKa of HXa) 2.5 b) 4 c) 8 d) 12

5) At which point is [HX] > [X-]?

a) A b) B c) C d) D

6) At which point is [HX] = [X-]?

a) A b) B c) C d) D

7) At which point(s) could the solution being titrated act as a buffer?a) only B b) only A, B c) only A, B, C d) A, B, C, D

Do 24 and 25 later

Based on #26

Based on #27:Which molecule has the smallest bond angle?a) CH4 b) NH3 c) H2O d) CO2

Which molecule has the largest bond angle?a) CH4 b) NH3 c) H2O d) CO2

Based on 29-31

A certain reaction: A(aq) + B(aq) C(aq) is studied. A is blue, B is colorless, and C is yellow. The reaction is 0-order with respect to [B]. A 5.0 mL sample of 0.001 Molar A is added to a 5.0 mL sample of 0.40 Molar B and mixed thoroughly. 1 mL of this mixture is added to a cuvette which is then placed in a spectrophotometer. The reaction progress is documented. The following results were obtained. Time (s) 0 10 20 30 40 50 60 70 80Absorbance of A

0.80 0.64 0.51 0.40 0.32 0.25 0.20 0.16 0.13

Approximately how much time was needed for 75% of the initial amount of A to react?a) 10 sec b) 30 sec c) 60 sec d) 80 sec

How would the initial rate of reaction change if the solution of A were diluted by a factor of 3 before being added to the solution of B?a) The rate would not be affected b) the rate would increase c) the rate would decrease d) the rate would decrease only if the solution of B were also diluted before being mixed with A.

The student wants to record run the experiment with the greatest sensitivity for A. The data shown above were obtained for the absorbance of A and C between the wavelengths of 200 and 800 nm. What is the best wavelength to use?a) 250 nm b) 400 nm c) 600 nm d) 680 nm

(Edye’s added questions)What is the order of the reaction with respect to A?a) 0 order b) 1st order c) 2nd order d) it cannot be determined from the data.

Based on #32

CH4(g) + H2O(g) CO(g) + 3 H⇌ 2(g) Kp = 7.7 x 1024 at 298 K

4 moles gaseous methane and 4 moles gaseous water are added to a previously evacuated rigid container. The mixture is sparked and allowed to react according to the equation above. At 298K, which of the following is true at equilibrium?a) [CH4] =[H2O] = [CO] and [H2]>[CO]b) [CH4] =[H2O] = [CO] and [H2] < [CO]c) [H2] > [CO] > [CH4]d) [CH4] =[H2O] and [H2] < [CO]

SO2(g) + NO2(g) NO(g) + SO⇌ 3(g) Kc = 85.0 at 460 °C4 moles gaseous SO2 and 4 moles gaseous NO2 are added to a previously evacuated rigid container. The mixture reacts according to the equation above. At 460oC, which of the following is true at equilibrium?a) [SO2] =[NO2] = [NO] = [SO3]b) [SO2] =[NO2], [NO] = [SO3], and [NO] > [SO2]c) [SO2] =[SO3], and [NO] > [SO2]d) [SO2] =[NO2], [NO] = [SO3], and [NO] < [SO2]

CH4(g) + H2O(g) CH⇌ 3OH(g) + H2(g) Kc = 2.8 x 10−21

4 moles gaseous CH4 and 4 moles gaseous H2O are added to a previously evacuated rigid container. The mixture reacts according to the equation above. Which of the following is true at equilibrium?a) [CH4] =[ H2O] = [CH3OH] = [H2]b) [CH4] =[ H2O], [CH3OH] = [H2], and [CH3OH] > [CH4]b) [CH4] =[ H2O], and [CH3OH] > [CH4]b) [CH4] =[ H2O], and [CH3OH] < [CH4]

Based on #33

Compound KspPbBr2 7 x 10-6

CuBr 6 x 10-9

AgBr 4 x 10-13

HgBr2 6 x 10-20

A 10.0 L container has a [CuNO3] = 0.0002 Molar and a [Pb(NO3)2] = 0.01 molar. 0.009 moles NaBr is added to the container, according to the data in the table above, what will happen?a) only PbBr2 will precipitateb) only CuBr will precipitatec) both PbBr2 and CuBr will precipitated) neither PbBr2 or CuBr will precipitate

A 10.0 L container has [Hg(NO3)2] = 0.0001 Molar and [AgNO3] = 0.0001 molar. 1 x 10-7 moles NaBr is added to the container. According to the data in the table above, what will happen?a) only HgBr2 will precipitateb) only AgBr will precipitatec) both HgBr2 and AgBr will precipitated) neither HgBr2 or AgBr will precipitate

A 10.0 L container has [Hg(NO3)2] = 0.0001 Molar and [AgNO3] = 0.00001 molar. 1 x 10-7 moles NaBr is added to the container. According to the data in the table above, what will happen?a) only HgBr2 will precipitateb) only AgBr will precipitatec) both HgBr2 and AgBr will precipitated) neither HgBr2 or AgBr will precipitate

Based on #34

The pH of a 0.01 M HCN solution (Ka = 6 x 10-10) would be approximatelya) 1 – 2 b)3-4 c) 5-6 d) 6-7

The pH of a 0.01 M HClO solution (Ka = 3 x 10-8) would be approximatelya) 1 – 2 b)3-4 c) 4-5 d) 5-6

The pH of a 0.1 M CH3COOH solution (Ka = 2 x 10-5) would be approximatelya) 1 – 2 b)2-3 c) 4-5 d) 6-7

Based on #35 PES problem

The photoelectron spectra for Fluorine and neon are shown above. Which of the following answers provides the correct set of peaks for fluorine, and correct justification?a) The solid line peaks represent fluorine. This is true because the solid peaks are slightly to the left of the dashed peaks and fluorine is to the left of neon in the periodic tableb) The solid line peaks represent fluorine. This is true because fluorine has fewer protons than neon.c) The dashed line peaks represent fluorine. This is true because neon’s 3p sublevel has 6 electrons, whereas fluorine’s 3p sublevel has only 5 electrons, as shown on the peaks at approximately 4 MJ/mold) The dashed line peaks represent fluorine. This is true because neon has more protons than fluorine.

The photoelectron spectra for chlorine and argon are shown above. Which of the following answers provides the correct set of peaks for chlorine, and correct justification?a) The solid line peaks represent chlorine. This is true because the solid peaks are slightly to the left of the dashed peaks and chlorine is to the left of argon in the periodic tableb) The solid line peaks represent chlorine. This is true because chlorine has fewer protons than argon.c) The dashed line peaks represent chlorine. This is true because argon’s 2p sublevel has 6 electrons, whereas chlorine’s 2p sublevel has only 5 electrons, as shown on the peaks at approximately 2 MJ/mold) The dashed line peaks represent chlorine. This is true because argon has more protons than chlorine.

The photoelectron spectra for the 1s and 2s sublevels for argon and neon are shown above. One element’s peaks are represented by dashed lines; the other element’s peaks are represented by solid lines. Which of the following is the correct element with the correct sublevel belonging to the element?a) A is the 1s sublevel of neonb) B is the 1s sublevel of neonc) C is the 1s sublevel of argond) D is the 1s sublevel of argon

A B C D

A B C D

The photoelectron spectra for the 1s and 2s sublevels for argon and neon are shown above. One element’s peaks are represented by dashed lines; the other element’s peaks are represented by solid lines. Which of the following is a correct statement with correct justification?a) peak A represents the 1s sublevel of neon. This is true because neon is smaller than argonb) peak A represent the 1s sublevel of argon. This is true because argon has more protons than neona) peak C represents the 1s sublevel of neon. This is true because neon is smaller than argonb) peak C represent the 1s sublevel of argon. This is true because argon has more protons than neon

Based on #36

A rigid 10.0 L container holds neon gas at a very high pressure. The measured pressure is much larger than the pressure predicted by the ideal gas law. Which of the following is the best explanation for this?a) neon atoms break into two boron atoms at high pressureb) at high pressure, neon atoms are very attracted to one another, causing the atoms to hit the walls of their container less often than if they were not attracted to one anotherc) the volume of the neon atoms is too large a fraction of the volume of the container to be negligibled) none of the above

A rigid 10.0 L container holds water vapor at a temperature very close to water’s boiling point. The measured pressure is smaller than the pressure predicted by the ideal gas law. Which of the following is the best explanation for this?a) water molecules break into hydrogen and oxygen molecules. b) water molecules are very attracted to one another, causing the molecules to hit the walls of their container less often and with less force c) the volume of the water molecules is too large a fraction of the volume of the container to be negligibled) none of the above

Based on #37 and 39

MgO(s) + C(graphite) Mg(s) + CO(g)

ΔH = 490 kJ/molRXN ΔS = 200 J/( molRXN K)

Two trials for the reaction above are carried out, and the heat flow is measured using a calorimeter. In the first trial, 1.2 g graphite reacts with 4.0 grams MgO (molar mass 40.). In the second trial, 1.2 g graphite reacts with 8.0 g MgO. In both trials, the same mass of magnesium is produced. Which of the following shows the correct limiting reactant and the correct amount of heat needed for the reaction?

Limiting reactant Heat required (kJ)a) C 49b) C 98c) MgO 49d) MgO 298

Which of the following statements about the thermodynamic favorability at 25oC about the reaction is correct?a) The reaction is not thermodynamically favorableb) The reaction is thermodynamically favorable and is driven by the entropy change onlyc) The reaction is thermodynamically favorable and is driven by the enthalpy change onlyd) The reaction is thermodynamically favorable and is driven by both enthalpy and entropy changes.

2 Mg(s) + O2(g) 2 MgO(s) Ho = -1200 kJ/molRXN So = -220 J/( molRXN K)

Two trials for the reaction above are carried out, and the heat flow is measured using a calorimeter. In the first trial, 2.4 grams Mg reacts with 3.2 grams O2. In the second trial, 2.4 g Mg reacts with 6.4 g O2. In both trials, the same mass of magnesium oxide is produced. Which of the following shows the correct limiting reactant and the correct amount of heat produced by the reaction?

Limiting reactant Heat produced (kJ)a) Mg 60.b) Mg 120c) O2 60.d) O2 120


2 H2O(l) + O2(g) → 2 H2O2(g) HΔ o = 200 kJ/ molRXN; SΔ o = -120 J/(K molRXN)

Two trials for the reaction above are carried out, and the heat flow is measured using a calorimeter. In the first trial, 1.8 grams water reacts with 3.2 grams O2. In the second trial, 3.2 g water reacts with 3.2 g O2. In both trials, the same mass of hydrogen peroxide is produced. Which of the following shows the correct limiting reactant and the correct amount of heat produced by the reaction?

Limiting reactant Heat required (kJ)a) H2O 20b) H2O 40c) O2 20d) O2 40


2 NaHCO3(s) g Na2CO3(s) + CO2(g) + H2O(g). Horxn = 130 kJ/molRXN and So

rxn = 320 J/( molRXN K)

Which of the following statements about the thermodynamic favorability at 500 K about the reaction is correct? (assume H and S remain the same at 500K as they are at 298 K.)a) The reaction is not thermodynamically favorableb) The reaction is thermodynamically favorable and is driven by the entropy change onlyc) The reaction is thermodynamically favorable and is driven by the enthalpy change onlyd) The reaction is thermodynamically favorable and is driven by both enthalpy and entropy changes.

2 NaHCO3(s) g Na2CO3(s) + CO2(g) + H2O(g). Horxn = 130 kJ/molRXN and So

rxn = 320 J/( molRXN K)

Which of the following statements about the thermodynamic favorability at 300 K about the reaction is correct? a) The reaction is not thermodynamically favorableb) The reaction is thermodynamically favorable and is driven by the entropy change onlyc) The reaction is thermodynamically favorable and is driven by the enthalpy change onlyd) The reaction is thermodynamically favorable and is driven by both enthalpy and entropy changes.

Based on #38

10 NaOH(aq) + 2 Cr(OH)3(s) + 3 Br2(g) 2 Na2CrO4(aq) + 8 H2O(l) + 6 NaBr(aq)

Atoms or ions of which element are reduced in the reaction above?a) Cr: each ion gains 3 electronsb) Na: each ion gains 1 electronc) Br: each atom gains 1 electrond) H: each ion gains 1 electron

Atoms or ions of which element are oxidized in the reaction above?a) Cr: each ion loses 3 electronsb) Na: each ion loses 1 electronc) Br: each atom loses 1 electrond) H: each ion gains 1 electron

6 HCl + 2 KMnO4 + 5 HCOOH 2 MnCl2 + 8 H2O + 5 CO2 + 2 KCl

Atoms or ions of which element are reduced in the reaction above?a) Mn: each atom gains 5 electronsb) C: each atom gains 2 electronsc) O: each atom gains 2 electronsd) Cl: each ion gains 1 electron

Atoms or ions of which element are oxidized in the reaction above?a) Mn: each atom loses 5 electronsb) C: each atom loses 2 electronsc) O: each atom loses 2 electronsd) Cl: each ion loses 1 electron

2 HCl + H2O2 + 2 FeCl2 2 FeCl3 + 2 H2O

Atoms or ions of which element are reduced in the reaction above?a) H: each ion atom gains 1 electronb) Cl: each ion gains 1 electronsc) O: each atom gains 1 electrond) Fe: each ion gains 1 electron

Atoms or ions of which element are oxidized in the reaction above?a) H: each ion atom loses 1 electronb) Cl: each ion loses 1 electronsc) O: each atom loses 1 electrond) Fe: each ion loses 1 electron

Based on #40

Bond Bond Energy

H-H 430O=O 500O-H 470

2 H2(g) + O2(g) 2 H2O (g)What will the drawing of the energy vs. reaction coordinate diagram look like for the above reaction?a) The reactants will be 520 kJ higher than the productsb) The reactants will be 520 kJ lower than the productsc) The reactants will be 420 kJ higher than the productsd) The reactants will be 420 kJ lower than the products

Bond Bond EnergyH-H 430

950N-H 390

N2 (g) + 3 H2(g) 2 NH3 (g)What will the drawing of the energy vs. reaction coordinate diagram look like for the above reaction?a) The reactants will be 1360 kJ higher than the productsb) The reactants will be 1360 kJ lower than the productsc) The reactants will be 230 kJ higher than the productsd) The reactants will be 230 kJ lower than the products

Bond Bond EnergyH-H 430F-F 160H-F 570

H2(g) + F2(g) 2 HF (g)What will the drawing of the energy vs. reaction coordinate diagram look like for the above reaction?a) The reactants will be 20 kJ higher than the productsb) The reactants will be 20 kJ lower than the productsc) The reactants will be 540 kJ higher than the productsd) The reactants will be 540 kJ lower than the products

Base on #41Ionization Energy

(kJ/mol)

1st 4962nd 4,5623rd 6,9124th 9,5435th 13,3536th 16,6107th 20,114

Based on the information in the table above, what would the most likely formula be for the unknown substance with chlorine?a) XCl b) XCl2 c) XCl3 d) X2Cl

Based on the information in the table above, what would the most likely formula be for the unknown substance with sulfur?a) XS b) XS2 c) X2S3 d) X2S

Based on the information in the table above, what would the most likely formula be for the unknown substance with nitrogen?a) XN b) X3N c) XN3 d) X3N2

Ionization Energy (kJ/mol)

1st 7382nd 14513rd 77334th 10,5405th 13,6306th 17,9957th 21,703




Ionization Energy (kJ/mol)

1st 578

2nd 18173rd 27454th 11,5755th 14,8306th 18,3767th 23,293




Based on #42

2 NO(g) + Cl2(g) 2 NOCl (g) Kp = 2 x 103 at 25oC

Samples of each of the above chemicals are added to a 10. L previously evacuated rigid container at 25oC until each has a partial pressure of 0.1 atm. The molecules are allowed to react until equilibrium is attained. At equilibrium, which species will have the highest pressure?a) only NO b) only Cl2 c) NOCl d) both NO and Cl2

Samples of each of the above chemicals are added to a 10. L previously evacuated rigid container at 25oC until each has a partial pressure of 0.1 atm. The molecules are allowed to react until equilibrium is attained. At equilibrium, which species will have the lowest pressure?a) only NO b) only Cl2 c) only NOCl d) both NO and Cl2

N2(g) + 3H2(g) 2 NH3(g) Kp = 5 x 105 at 25oC.

Pure samples of each of the above chemicals are added to a 10. L previously evacuated rigid container so that each has an initial partial pressure of 0.1 atm at 25oC. The chemicals are allowed to react until equilibrium is attained. At equilibrium, which species will have the lowest concentration?a) only N2 b) only H2 c) only NH3 d) both N2 and H2

Pure samples of each of the above chemicals are added to a 10. L previously evacuated rigid container so that each has an initial partial pressure of 0.1 atm at 25oC. The chemicals are allowed to react until equilibrium is attained. At equilibrium, which species will have the highest concentration?a) only N2 b) only H2 c) only NH3 d) both N2 and H2

2 NOCl (g) 2 NO(g) + Cl2(g) Kc = 2 x 10-5 at 35oC

0.1 moles of each of the above chemicals are added to a 10. L previously evacuated rigid container at 25oC. The chemicals are allowed to react until equilibrium is attained. At equilibrium, which species will have the highest concentration?a) only NOCl b) only NO c) only Cl2 d) both NO and Cl2

0.1 moles of each of the above chemicals are added to a 10. L previously evacuated rigid container at 25oC. The chemicals are allowed to react until equilibrium is attained. At equilibrium, which species will have the lowest concentration?a) only NOCl b) only NO c) only Cl2 d) both NO and Cl2

2 A (g) + 3 B (g) C (g) + 2 D (g) at 15oC, Kc = 2 x 10-5

For the hypothetical experiment above, 0.1 moles of each of the above chemicals are added to a 10. L previously evacuated rigid container at 25oC. The chemicals are allowed to react until equilibrium is attained. At equilibrium, which species will have the lowest concentration?a) A b) B c) C d) D

For the hypothetical experiment above, 0.1 moles of each of the above chemicals are added to a 10. L previously evacuated rigid container at 25oC. The chemicals are allowed to react until equilibrium is attained. At equilibrium, which species will have the highest concentration?a) A b) B c) C d) D

2 A (g) + 3 B (g) C (g) + 2 D (g) at 15oC, Kc = 2 x 105

For the hypothetical experiment above, 0.1 moles of each of the above chemicals are added to a 10. L previously evacuated rigid container at 25oC. The chemicals are allowed to react until equilibrium is attained. At equilibrium, which species will have the lowest concentration?a) A b) B c) C d) D

For the hypothetical experiment above, 0.1 moles of each of the above chemicals are added to a 10. L previously evacuated rigid container at 25oC. The chemicals are allowed to react until equilibrium is attained. At equilibrium, which species will have the highest concentration?a) A b) B c) C d) D

Based on #43

Y

A pure solid substance is heated at 2.0 atm, forming liquid and then vapor. Which of the following correctly assigns the sign for the change in enthalpy and entropy for the process when moving from point X to point Y?

Ho So

a) Positive Positiveb) Negative Negativec) Positive Negatived) Negative Positive

A pure solid substance is heated at 2.0 atm, forming liquid and then vapor. Which of the following correctly assigns the sign for the change in enthalpy and entropy for the process when moving from point X to point Y?

Ho So


Y

YX

A pure gaseous substance is cooled at 2.0 atm, forming liquid and then solid. Which of the following correctly assigns the sign for the change in enthalpy and entropy for the process when moving from point X to point Y?

Ho So


A pure gaseous substance is cooled at 2.0 atm, forming liquid and then solid. Which of the following correctly assigns the sign for the change in enthalpy and entropy for the process when moving from point X to point Y?

Ho So


Based on #44-47

X

Y

N2(g) + 3 H2(g) 2 NH3 (g) Ho = -92 kJ/molRXN Kp = 5 x 105 at 298 K.

Nitrogen and hydrogen gases are added to a previously evacuated 10.0 L rigid insulated container at 25oC to obtain initial partial pressures of 1.0 atm each. They are allowed to react until equilibrium is reached.

How will the temperature inside the container be affected as the reaction proceeds?a) the temperature will steadily increase until equilibrium is achieved because the reaction is exothermicb) the temperature will steadily decrease until equilibrium is achieved because the reaction is endothermicc) the temperature will first increase, then because the total number of gas particles decreases, the temperature will decrease according to PV=nRT.d) the temperature will first decrease, then slowly increase until equilibrium is achieved

What can you conclude about the sign of So?a) So must be greater than zero because ngas= -2b) So must be greater than zero because K > 1c) So must be less than zero because ngas = -2d) So must be less than zero because K > 1

What can you conclude about the relative strength of the bond energies of the reactants and products?a) The bond energy of the reactants is greater than the bond energy of the products because according to the sign of Ho, more energy is released from the reactant bonds breaking than is put in when product bonds are formed.b) The bond energy of the reactants is greater than the bond energy of the products because K > 1c) The bond energy of the reactants is less than the bond energy of the products because according to the sign of Ho, less energy is put into breaking the reactant bonds than is given off when product bonds are formed.d) There is not enough information given to make a conclusion about the relative strength of the bond energies of the reactants and products.

If the reaction could go to completion, and the temperature brought back to 25oC, what would the final total pressure in the container be?a) 0.7 atm b) 1.0 atm c) 1.3 atm d) 2.0 atm

2 NO(g) + Cl2(g) 2 NOCl (g) Ho = -80 kJ/molRXN Kp = 2 x 103 at 25oC

Nitrogen monoxide and chlorine gases are added to a previously evacuated 10.0 L rigid insulated container at 25oC to obtain initial partial pressures of 1.0 atm each. They are allowed to react until equilibrium is reached.

How will the temperature inside the container be affected as the reaction proceeds?a) the temperature will steadily increase until equilibrium is achieved because the reaction is exothermicb) the temperature will steadily decrease until equilibrium is achieved because the reaction is endothermicc) the temperature will first increase, then because the total number of gas particles decreases, the temperature will decrease according to PV=nRT.d) the temperature will first decrease, then slowly increase until equilibrium is achieved

What can you conclude about the sign of So?a) So must be greater than zero because ngas= -1b) So must be greater than zero because K > 1c) So must be less than zero because ngas = -1d) So must be less than zero because K > 1

What can you conclude about the relative strength of the bond energies of the reactants and products?a) The bond energy of the reactants is greater than the bond energy of the products because according to the sign of Ho, more energy is released from the reactant bonds breaking than is put in when product bonds are formed.b) The bond energy of the reactants is greater than the bond energy of the products because K > 1c) The bond energy of the reactants is less than the bond energy of the products because according to the sign of Ho, less energy is put into breaking the reactant bonds than is given off when product bonds are formed.d) There is not enough information given to make a conclusion about the relative strength of the bond energies of the reactants and products.

If the reaction could go to completion, and the temperature brought back to 25oC, what would the final total pressure in the container be?a) 0.5 atm b) 0.7 atm c) 1.0 atm d) 2.0 atm

2 A2(g) + B2(g) 2 AB (g) + 2 A(g) Ho = 80 kJ/molRXN

Gases A2 and B2 are added to a previously evacuated 10.0 L rigid insulated container at 25oC to obtain initial partial pressures of 1.0 atm each. They are allowed to react, and the reaction essentially goes to completion.

How will the temperature inside the container be affected as the reaction proceeds?

a) the temperature will steadily increase until equilibrium is achieved because the reaction is exothermicb) the temperature will steadily decrease until equilibrium is achieved because the reaction is endothermicc) the temperature will first increase, then because the total number of gas particles decreases, the temperature will decrease according to PV=nRT.d) the temperature will first decrease, then slowly increase until equilibrium is achieved

What can you conclude about the sign of So?a) So must be greater than zero because ngas= -1b) So must be greater than zero because Go<0 and Ho>0c) So must be less than zero because ngas = +1d) So must be less than zero because K > 1

What can you conclude about the relative strength of the bond energies of the reactants and products, with correct justification?a) The bond energy of the reactants is greater than the bond energy of the products because according to the sign of Ho, more energy is needed to break reactant bonds than is released when product bonds are formed.b) The bond energy of the reactants is less than the bond energy of the products because K > 1c) The bond energy of the reactants is less than the bond energy of the products because according to the sign of Ho, more energy is given off when breaking the reactant bonds than is put in when product bonds are formed.d) The bond energy of the reactants is more than the bond energy of the products because 3 bonds are forming only 2 bonds.

If the reaction goes to completion, and the temperature brought is back to 25oC, what would the final total pressure in the container be?a) 0.5 atm b) 1.0 atm c) 2.0 atm d) 2.5 atm

Based on # 48

Base Concetration (M)

pH

A 0.1 13B 1.0 11C 2.0 11

Which of the following ranks the 3 bases above from weakest to strongest base?a) C < B < A b) A < B < C c) A < C < B d) B < C < A


pH

A 3.0 10B 2.0 10C 1.0 13

Which of the following ranks the 3 bases above from weakest to strongest base?a) C < B < A b) A < B < C c) A < C < B d) B < C < A


pH

A 3.0 13B 2.0 8C 0.01 12

Which of the following ranks the 3 bases above from weakest to strongest base?a) B < C < A b) A < B < C c) A < C < B d) B < A < C


pH

A 0.1 1B 1.0 3C 2.0 3

Which of the following ranks the 3 monoprotic acids above from strongest to weakest acid?a) C > B > A b) A > B > C c) A > C > B d) B > C > A


pH

A 3.0 1.5B 2.0 1.5C 1.0 1.2

Which of the following ranks the 3 monoprotic acids above from strongest to weakest acid?a) C > B > A b) A > B > C c) A > C > B d) B > C > A


pH

A 3.0 1B 2.0 2C 0.01 2

Which of the following ranks the 3 monoprotic acids above from strongest to weakest acid?a) B > C > A b) C > A > B c) A > C > B d) B > A > C Based on #49

Based on #50

3 AgNO3(aq) + Al(s) ---> Al(NO3)3(aq) + 3 Ag(s)If 100. mL of 0.40 M AgNO3 is added to 0.270 g Al and allowed to react completely, which of the following is/are true?a) aluminum is the limiting reactant and 0.030 moles silver nitrate remainb) aluminum is the limiting reactant and 0.020 moles silver nitrate remain

c) 0.040 moles silver are producedd) 0.030 moles silver are produced

3 AgNO3(aq) + Al(s) ---> Al(NO3)3(aq) + 3 Ag(s)If 100. mL of 0.80 M AgNO3 is added to 0.540 g Al and allowed to react completely, which of the following is/are true?a) aluminum is the limiting reactant and 0.030 moles silver nitrate remainb) aluminum is the limiting reactant and 0.020 moles silver nitrate remainc) 0.080 moles silver are producedd) 0.040 moles aluminum nitrate are produced

Documents

WARNING: THIS WEBSITE DEFIES THE SECOND LAW OF … · Web viewTwo trials for the reaction above are carried out, and the heat flow is measured using a calorimeter. In the first trial,