Ch. 3 Honors Chem HW #11 HC 1 of 4 A2) An element is a mixture of two isotopes. One isotope of the element has an atomic mass of 34.96885 amu and has a relative abundance of 75.53%. The other isotope has an atomic mass of 36.96590 amu. Calculate the average atomic mass and identify the element.

A4) The element europium exists in nature in two isotopes. 151Eu has a mass of 150.9196 amu and 153Eu has a mass of 152.9209 amu. The average atomic mass of europium is 151.96 amu. Calculate the relative abundance of the two europium isotopes.

B12) Aspartame, C14H18N2O5, is an artificial sweetener that is 160 times sweeter than sucrose (table sugar) when dissolved in water. a) Calculate the molar mass of aspartame. b) How many moles are present in 10.0 g of aspartame?

c) How many grams are in 1.56 mol of aspartame?

d) How many molecules are in 5.0 mg aspartame?

e) How many atoms of nitrogen are in 1.2 g aspartame? #11 HC 4 of 4

f) How many grams are in 1.0 X109 molecules of aspartame?

b) C4H6O2 (methyl acrylate, from which Plexiglas is made)

C4) Calculate the mass percent of carbon for each of the following substances and #12 HC 3 of 5 then arrange the substances in order of increasing mass percent of carbon. Caffeine, C8H10N4O2 Sucrose, C12H22O11 Ethanol, C2H5OH

C5) Vitamin B12, cyanocobalamin, is essential for human nutrition. Since vitamin B12 is in animal tissue, but not in higher plants, vegetarians may become deficient in vitamin B12. Cyanocobalamin contains 4.34% cobalt by mass. Calculate the molar mass of cyanocobalamin, if there is one cobalt atom in each molecule of cyanocobalamin.

D1) Give the empirical formula for each of the following compounds. #12 HC 4 of 5 a) vitamin C, C6H8O6 b) benzene, C6H6 c) acetylene, C2H2 d) phosphorus pentoxide, P4O10 e) glucose, C6H12O6 f) acetic acid, HC2H3O2

D4) The compound adrenalin contains 56.79% C, 6.56% H, 28.37% O and 8.28% N by mass. What is the empirical formula for adrenaline?

D6) A compound that contains only nitrogen and oxygen is 30.4% N by mass. #12 HC 5 of 5 The molar mass of the compound is 92 g/mol. What is the empirical formula of the compound? What is the molecular formula of the compound?

C6) Fungal laccase, a blue protein found in wood-rotting fungi is 0.390% Cu by mass. #13 HC 1 of 6 If a fungal laccase molecule contains 4 copper atom, what is the molar mass of fungal laccase?

H2) Find the formula of the following hydrates: a) 0.737 g MgSO3 and 0.763 g H2O

c) 76.9 % CaSO3 and 23.1 % H2O #13 HC 3 of 6

b) Al(OH)3(s) + HCl(aq) → AlCl3(aq) + H2O(l)

double displacement

b) C6H6(l) + O2(g) → CO2(g) + H2O(g) #14 HC 2 of 7

combustion

e) FeO(s) + O2(g) → Fe2O3(s)

Synthesis #14 HC 4 of 7

E5) Balance the following equations and state the type: a) Cr(s) + S8(s) → Cr2S3(s)

synthesis

b) heat + NaHCO3(s) → Na2CO3(s) + CO2(g) + H2O(g)

(The “heat” can be ignored.)

decomposition

d) Eu(s) + HF(g) → EuF3(s) + H2(g) #14 HC 5 of 7

single displacement

F2) The compound cisplatin, Pt(NH3)2Cl2, has been studied extensively as an antitumor agent. Cisplatin is synthesized as follows: K2PtCl4(aq) + 2 NH3(aq) → Pt(NH3)2Cl2(s) + 2 KCl(aq) a) What mass of cisplatin, Pt(NH3)2Cl2, can be made from 100. g of K2PtCl4?

b) What mass of KCl can be made from 100. g of K2PtCl4?

G1) When a mixture of silver metal and sulfur is heated, silver sulfide is formed: #15 HC 2 of 3 heat + 16 Ag(s) + S8(s) → 8 Ag2S(s) a) What mass of Ag2S is produced from a mixture of 2.0 g Ag and 2.0 g S8?

b) What mass of which reactant is left unreacted?

G2) Mercury and bromine will react with each other to produce mercury II bromide: #15 HC 3 of 3 Hg(l) + Br2(l) → HgBr2(s) a) What mass of HgBr2 can be produced from the reaction of 10.0g Hg and 9.00 g Br2? What mass of which reagent is left unreacted?

b) What mass of HgBr2 can be produced from the reaction of 5.00 ml Hg (density = 13.6 g/ml) and 5.00 ml Br2 (density = 3.10 g/ml)?

G6) Aluminum burns in bromine, producing aluminum bromide: #16 HC 1 of 3 2 Al(s) + 3 Br2(l) → 2 AlBr3(s) In a certain experiment, 6.0 g Al was reacted with an excess of bromine to yield 50.3 g aluminum bromide (experimental yield). Calculate the theoretical and percent yields for this experiment.

G7) Consider the following unbalanced reaction: P4(s) + F2(g) → PF3(g) How many grams of F2 are needed to produce 120. g of PF3, if the reaction has a 78.1% yield?

D10) Many homes in rural America are heated by propane gas, a compound that #16 HC 2 of 3 only contains carbon and hydrogen. Complete combustion of a sample of propane produced 2.641 g of carbon dioxide and 1.442 g of water as the only products. Find the empirical formula of propane.

D13) A compound contains only carbon, hydrogen, and oxygen. #16 HC 3 of 3 Combustion of 10.68 mg of the compound yields 16.01 mg CO2 and 4.37 mg H2O. The molar mass of the compound is 176.1 g/mol. What are the empirical and molecular formulas of the compound?