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Chemistry (3) Interim Assessment (3) Page 1
Name ____________________________________ Date ____________________ ID __________________
Chemistry (3) Interim Assessment Third Grading Period
1. Oxidation-reduction reactions involve electrons being either lost or gained. Which of the following is an example of an element undergoing the oxidation process?
F + e- F-1
Mg Mg+2 + 2e-
Br-1 + 2e- Br2
HOH H+1 + OH-1
2. In the following redox equation, what is the oxidation number for lead (Pb) on the product side of the equation?
Pb + CuC12 Cu + PbC14
0
+1
+2
+4
3. In a redox reaction a substance is reduced by gaining electrons. In the equation below, which substance is reduced?
KI + HgF4 KF + HgI2
K
I
Hg
F
Chemistry (3) Interim Assessment (3) Page 2
4. Below you will find four chemical equations, only one of which is an example of an oxidation-reduction reaction. Identify the oxidation-reduction reaction.
MnS + FeO MnO + FeS
CaCO3 CaO + CO2
CrC13 + 3 Li 3 LiC1 + Cr
H2SO3 + 2 KOH K2SO3 + 2 HOH
5. Often metals will corrode when exposed to air and water. Three of the four statements below are examples of the corrosion process. Identify the one that is not the corrosion of a metal.
A shiny but inexpensive silver ring soon begins to turn black.
The statue of liberty, which is covered with copper, becomes green in color.
The post of a car battery (lead) becomes coated with a white powdery substance.
When placed in a container of acid, a piece of Magnesium completely dissolves.
6. A solid compound is placed in a beaker to which 100 ml of water is added. The compound is stirred until it completely dissolves. Which of the following would indicate that an endothermic reaction has occurred?
The water changes from clear to a light yellow color.
A drop in temperature is observed.
An increase in temperature is observed.
A solid substance forms in the bottom of the container.
7. You heated 500 g of silver from 20 °C to its melting point of 962 °C. The energy (q) need to accomplish this is 113, 040 J. Using the formula provided, calculate the specific heat (C) of silver in J/(g x °C).
q = m x T x C
0.24
1.60
2.33
4.25
Chemistry (3) Interim Assessment (3) Page 3
8. Hess's Law makes it possible to measure the heat of reaction indirectly. Using the reaction information provided, determine the heat of reaction ( H) using the formula provided. NaHCO3 NaOH + CO2
Hf° NaHCO3 = -1520 kJ
Hf° NaOH = -840 kJ
Hf° CO2 = -393 kJ
H = Hf°(products) - Hf°(reactants)
-2,753 kJ
-1,967 kJ
287 kJ
53 kJ
9. Four different samples (10 grams each) of CuCl2 shown below are added to four flasks, each containing 150 ml of a prepared solution containing another compound. The samples are of different size as indicated. As the expected chemical reactions occur, and based on what you know about reaction rates of chemical reactions, which sample of CuCl2 would cause the reaction to occur the fastest?
Sample A
Sample B
Sample C
Sample D
Chemistry (3) Interim Assessment (3) Page 4
10. The above graph shows the relationship between temperature and the reaction rate of a chemical change. Which statement best summarizes this relationship?
As the temperature increases the reaction rate tends to increase.
Increasing the temperature will cause the reaction rate to decrease.
Temperature and reaction rate have an inverse relationship.
Reaction rate and temperature are mirror images of one another.
11. Entropy is a measure of the disorder of a system. Scattered particles have higher entropy than gathered particles. Which of the conditions listed below shows a movement towards a lower level entropy?
A liquid changing into a solid.
A solid changing into a liquid.
A liquid evaporating into a vapor.
A solid being broken into pieces.
Chemistry (3) Interim Assessment (3) Page 5
12. The graph below shows the relationship between the energy released during a chemical reaction (measured in kJ) based on the concentration of a compound in solution measured in grams per liter of solution.
Based on the information in the graph, infer how many kJ were released when 400 grams of the compound was involved in the reaction. To show the kJ released, where should you draw the line in the blank column?
15,000 kJ
20,000 kJ
25,000 kJ
30,000 kJ
Chemistry (3) Interim Assessment (3) Page 6
13. A weather balloon containing 200 liters of a lighter than air gas was released into the atmosphere. The air pressure that day was 100 kPa. The balloon will burst when the volume of gas reaches 1,200 liters. Calculate the pressure when the balloon will burst and, use the information in the chart below to determine the altitude where this happens. P1 V1 = P2 V2
Altitude in feet Air pressure in kPa 10,000 80 20,000 60 30,000 40 40,000 20 50,000 10 60,000 5 70,000 2 80,000 1
Based on your calculations, and information contained in the chart, the balloon will bust at approximately
20,000 ft.
40,000 ft.
60,000 ft.
80,000 ft.
14. Norma is cooking a pot roast using a pressure cooker. A pressure cooker is a sealed pot that uses high heat and pressure to cook foods. When she began the cooking process the cooker contained 6 liters of air at 27 °C and the pressure inside the cooker was 102 kPa. After cooking the roast, the temperature of the air inside was 160 °C and the pressure was 240 kPa. How many liters of air remained in the cooker? * Remember to make the necessary temperature conversions.
5.8
4.5
3.7
2.6
Chemistry (3) Interim Assessment (3) Page 7
15. The Ideal Gas Law, also known as the Universal Gas Law, is represented by the formula: P x V = n x R x T
R is a constant with the value of 8.31 (L x kPa) / (K x mol.) Based on the Ideal Gas Law, what is the approximate volume of a 2.75 moles of NO2 contained in a tank with a pressure of 101 kPa and at a temperature of 310 K?
70 L
55 L
26 L
8 L
16. Which statement below correctly summarizes the relationship between the two factors?
As the pressure on a gas in a tank is increased three times, the volume of the gas increases three times as well.
When the temperature of a gas decreases by half, the pressure increases twice as much as the original pressure.
If the volume of a gas increased by a factor of six, the temperature must have increased by a factor of three.
Increasing the pressure on a gas by a factor of three reduces the volume to one- third the original volume.
2 H2O (liquid) 2 H2 (gas) + O2 (gas) S° = + 152.6 J/K 17. The above reaction has a standard entropy change as indicated. Notice that 2 molecules of water decompose to form 3 molecules of gases. Knowing that entropy indicates the disorder of a system, then the positive value for the standard entropy change tells you a
less ordered system was formed.
decrease in entropy was observed.
balanced state of entropy occurred.
more ordered system was formed.
Chemistry (3) Interim Assessment (3) Page 8
18. Magnesium reacts with hydrochloric acid according to the following equation: Mg + 2 HCl MgCl2 + H2
You have 10 grams of Mg and 500 ml of HCl in a one-liter container. If you wanted to increase the reaction rate, you could do a number of things. All of the following will accomplish this except one. Which action will not increase the reaction rate?
Add more magnesium to the acid.
Warm the liquid to near boiling.
Add more acid to the container.
Cut the magnesium into smaller pieces.
19. When steam condenses into liquid water an energy change has taken place. Based on what you have learned about changes in matter and the energy involved, this change will be classified as exothermic. Why?
Energy, in the form of heat, has been given off.
Energy, in the form of heat, has been absorbed.
Heat energy has caused a physical change to occur.
The temperature of the steam was higher than the water.
20. Three containers are filled with oil heated to, and maintained at, 210 °C.
Which statement below is a correct summary statement in regards to heat?
Container C has the highest temperature of the three containers.
All three containers took the same amount of time to reach 210 °C.
Container B contains more heat energy than the other two containers.
All three containers have the same amount of heat energy.
Chemistry (3) Interim Assessment (3) Page 9
21. A group of chemistry students were given a problem to solve. They obtained the needed equipment and materials and conducted the tests they thought were necessary to solve the problem. The group kept careful notes, organized the collected data and made a presentation of their findings to the class. Which part of the scientific method did they forget to follow?
state the problem
form a hypothesis
perform an experiment
communicate results
Growth in inches Day Chemical plant food
added Number of hours of
daylight Rainfall in
inches 1 1 2 ml 9.0 0 3 2 2 ml 9.1 0 8 5 2 ml 9.4 0 12 9 2 ml 9.5 1.2 18 15 2 ml 9.8 0 26 19 2 ml 10.0 0 37 22 2 ml 10.2 0.5 49 25 2 ml 10.3 .25 61 30 2 ml 10.4 0
22. Lynn wanted to see how fast she could grow a plant from its starting height of 3 inches. Lynn recorded the hours of daylight, ml of plant food added, and inches of rainfall for each day she made a height measurement. She recorded her findings in the chart above. Which data seems unreasonable?
Growth in inches
Chemical plant food
Number of hours of daylight
Rainfall in inches
Chemistry (3) Interim Assessment (3) Page 10
23. Which career listed below probably needs to know the most chemistry?
Oceanographer
X-ray technician
Geologist
Pharmacist
24. For a project in her science class, Sue compared the density of ten different liquids she had collected. Which would be the most appropriate method to display this comparison?
Line graph
Pie chart
Bar graph
Scatter plot
Name___________________________ Date___________________ ID ____________
Chemistry (3) Interim Assessment Third Grading Period
Answer Document
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Chemistry (2) Interim Assessment (2) Page 7
Ion Chart For use on IPC and Chemistry Interim Assessments
Common Monatomic Ions +1 +2 +3 +4 -3 -2 -1 Li Ba Al Pb N O F Na Mg Fe Sn P S Cl K Ca Cr As Se Br Rb Sr Mn I Cs Cu Co Cu Fe Ag Be
Hg Sn Co Mn Cr Pb Ni Zn
Common Polyatomic Ions
-1 Charge -2 Charge -3 Charge Formula Name Formula Name Formula Name C2H3O2 Acetate HPO4 Hydrogen
Phosphate PO3 Phosphite
HCO3 Hydrogen Carbonate
SO3 Sulfite PO4 Phosphate
HSO4 Hydrogen Sulfate
SO4 Sulfate
NO2 Nitrite CO3 Carbonate +1 Charge NO3 Nitrate CrO4 Chromate NH4 AmmoniumCN Cyanide Cr2O7 Dichromate OH Hydroxide SiO3 Silicate MnO4 Permanganate ClO2 Chlorite ClO3 Chlorate
13
Density =
( ) = ( )( )( )Speed =
Acceleration =
Momentum = mass × velocity
Force = mass × acceleration
Work = force × distance
Power =
% efficiency = × 100
Kinetic energy = (mass × velocity 2)
Gravitational potential energy = mass × acceleration due to gravity × height
Energy = mass × (speed of light) 2
Velocity of a wave = frequency × wavelength
Current =
Electrical power = voltage × current
Electrical energy = power × time
voltageresistance
12
work outputwork input
worktime
final velocity − initial velocitychange in time
distancetime
specificheat
change intemperature
mass ingrams
heat gained orlost by water
massvolume
FORMULA CHARTfor Grades 10–11 Science Assessment
Constants/Conversions
g = acceleration due to gravity = 9.8 m/s 2
c = speed of light = 3 × 10 8 m/s
speed of sound = 343 m/s at 20°C
1 cm 3 = 1 mL
1 wave/second = 1 hertz (Hz)
1 calorie (cal) = 4.18 joules
1000 calories (cal) = 1 Calorie (Cal) = 1 kilocalorie (kcal)
newton (N) = kgm/s 2
joule (J) = Nm
watt (W) = J/s = Nm/s
volt (V) ampere (A) ohm (Ω)
10
23
45
67
89
1011
1213
1415
1617
1819
20
Centim
etersD =
Q = (m)(∆T)(Cp)
s =
a =
p = mv
F = ma
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KE =
GPE = mgh
E = mc 2
v = f λ
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P = VI
E = Pt
VR
mv 2
2
WO
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Wt
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2526
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3738
3940
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5556
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7576
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510
610
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58.6
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