Practice questions for Chapter 8

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1 Practice questions for Chapter 8 2) How many atoms of nickel equal a mass of g? (Refer to the Periodic Table.) A) 1 B) 28 C) D) 59 E) 6.02 x 1023 Answer: E Section: 8.1 Avogadro's Number 6) What is the number of sulfur atoms that equal a mass of amu? A) 1 B) 16 C) 32 D) 6.02 x 1023 Section: 8.1 Avogadro's Number 9) What is the number of manganese atoms that equal a mass of g? A) 1 B) 25 C) 55 D) 6.02 x 1023 Section: 8.1 Avogadro's Number 13) Which of the following is equal to 1.00 mole of substance? A) 6.02 x 1023 sodium atoms, Na B) 6.02 x 1023 iodine molecules, I2 C) 6.02 x 1023 sodium iodide formula units, NaI D) all of the above Section: 8.2 Mole Calculations I 14) Which of the following is equal to 1.00 mole of substance? A) 6.02 x 1023 lithium atoms, Li B) 6.02 x 1023 fluorine molecules, F2 C) 6.02 x 1023 lithium fluoride formula units, LiF D) all of the above Section: 8.2 Mole Calculations I

2 17) How many molecules of methane are in mol of CH4 gas? A) 1.20 x 1023 molecules B) 1.20 x 1024 molecules C) 3.01 x 1022 molecules D) 3.01 x 1023 molecules E) 3.01 x 1024 molecules Section: 8.2 Mole Calculations I 20) How many moles of ammonia contain 1.51 x 1024 NH3 molecules? A) mol B) mol C) 2.51 mol D) 3.99 mol E) 25.1 mol Section: 8.2 Mole Calculations I 24) What is the molar mass of cholesterol, C27H45OH? A) g/mol B) g/mol C) g/mol D) g/mol E) g/mol Section: 8.3 Molar Mass 26) What is the molar mass of aluminum chlorate, Al(ClO3)3? A) g/mol B) g/mol C) g/mol D) g/mol E) g/mol Section: 8.3 Molar Mass 31) What is the mass of 4.50 x 1022 atoms of gold, Au? A) g B) g C) 13.3 g D) 14.7 g E) 2640 g Section: 8.4 Mole Calculations II 32) What is the mass of 3.30 x 1023 atoms of silver, Ag? A) g

3 B) 25.8 g C) 59.1 g D) 85.7 g E) 197 g Section: 8.4 Mole Calculations II 37) How many molecules of bromine liquid, Br2, have a mass equal to 31.8 g? A) 1.20 x 1023 molecules B) 1.51 x 1024 molecules C) 1.91 x 1025 molecules D) 2.40 x 1023 molecules E) 3.03 x 1024 molecules Section: 8.4 Mole Calculations II 43) What is the mass in grams of a single formula unit of silver chloride, AgCl? A) 1.16 x g B) 1.66 x g C) 2.38 x g D) 4.21 x 1021 g E) 8.61 x 1025 g Section: 8.4 Mole Calculations II 45) Which of the following gases occupies 22.4 L at STP? A) 1 mol hydrogen, H2 B) 1 mol nitrogen, N2 C) 1 mol of oxygen, O2 D) all of the above Section: 8.5 Molar Volume 46) Which of the following gases occupies 22.4 L at STP? A) 1 mol helium, He B) 1 mol neon, Ne C) 1 mol xenon, Xe D) all of the above Section: 8.5 Molar Volume 54) How many xenon atoms are in 10.0 L of Xe gas at STP? A) 1.35 x 1024 atoms B) 2.69 x 1021 atoms

4 C) 2.69 x 1023 atoms D) 6.02 x 1022 atoms E) 6.02 x 1024 atoms 55) How many hydrogen molecules are in 2.75 L of H2 gas at STP? A) 1.66 x 1024 molecules B) 2.19 x 1023 molecules C) 4.90 x 1024 molecules D) 7.39 x 1022 molecules E) 9.77 x 1021 molecules 59) What is the mass of 455 ml of ethane gas, C2H6, at STP? A) g B) g C) 2.95 g D) 10.2 g E) 65.9 g 66) What is the density of fluorine gas, F2, at STP? A) g/l B) g/l C) 1.18 g/l D) 1.70 g/l E) 22.4 g/l 70) If the density of an unknown gas is 1.96 g/l at STP, what is its molar mass? A) 11.4 g/mol B) 19.6 g/mol C) 22.4 g/mol D) 43.9 g/mol E) 196 g/mol 79) The formula for mustard gas used in chemical warfare is C4H8SCl2 ( g/mol). What is the percentage of carbon in the compound? A) 5.08% B) 7.55% C) 20.16%

5 D) 30.20% E) 44.57% Section: 8.7 Percent Composition 80) The formula for mustard gas used in chemical warfare is C4H8SCl2 ( g/mol). What is the percentage of hydrogen in the compound? A) 0.635% B) 5.08% C) 20.16% D) 30.20% E) 44.57% Section: 8.7 Percent Composition 89) If mol of lead combines with mol of sulfur, what is the empirical formula of the lead sulfide product? A) PbS B) Pb2S C) PbS2 D) Pb3S3 Section: 8.8 Empirical Formula 97) If g of tin metal reacts with g of fluorine gas, what is the empirical formula of the product? A) SnF B) SnF2 C) SnF4 D) SnF10 E) Sn2F3 Section: 8.8 Empirical Formula

6 Chapter 9 1) What term refers to the amount of product experimentally measured in a laboratory procedure? A) actual yield B) percent yield C) stoichiometric yield D) theoretical yield 4) What principle states that mass is neither gained or lost during a chemical reaction? A) Avogadro s theory B) law of combining volumes C) law of conservation of mass D) law of constant composition 5) What is the term for the substance in a chemical reaction that controls the maximum amount of product? A) limiting reactant B) limiting product C) maximum reactant D) maximum product 6) What term refers to a type of stoichiometry calculation that relates the masses of two substances according to a balanced chemical equation? A) mass-mass problem B) mass-volume problem C) mole-mole problem D) volume-volume problem 7) What term refers to a type of stoichiometry calculation that relates the mass of a substance to the volume of a gas according to a balanced chemical equation? A) mass-mass problem B) mass-volume problem C) mole-mole problem

7 D) volume-volume problem 8) What term refers to the mass of 1 mol of substance expressed in grams? A) gram-atomic mass B) gram-molecular mass C) gram-formula mass D) molar mass 9) What term refers to the volume occupied by 1 mol of any gas at STP? A) Avogadro s volume B) molar volume C) standard volume D) STP volume 11) What is the term for the actual yield compared to the theoretical yield expressed as a percent? A) experimental yield B) percent yield C) ratio yield D) stoichiometric yield 13) What is the term for the relationship of quantities (i.e., mass of substance or volume of gas) in a chemical reaction according to the balanced chemical equation? A) mass-mass problem B) mass-volume problem C) volume-volume problem D) stoichiometry 50) What is the mass of iron(iii) bromide ( g/mol) that yields g of silver bromide ( g/mol) precipitate? FeBr3(s) + AgNO3(aq) AgBr(s) + Fe(NO3)3(aq) A) g B) g C) g

8 D) g E) g Section: 9.4 Mass-Mass Problems 58) What is the mass of aluminum metal that reacts to give 11.1 g of manganese metal? MnO2(l) + Al(l) A) 3.64 g B) 4.09 g C) 5.45 g D) 7.27 g E) 8.18 g Section: 9.4 Mass-Mass Problems Mn(l) + Al2O3(s) 59) What is the mass of hydrogen gas released from 2.70 g of aluminum metal and hydrochloric acid? Al(s) + HCl(aq) AlCl3(aq) + H2(g) A) g B) g C) g D) g E) g Section: 9.4 Mass-Mass Problems 97) Considering the limiting reactant, what is the mass of manganese produced from 25.0 g of manganese(iv) oxide (86.94 g/mol) and 25.0 g of aluminum metal? 3 MnO2(l) + 4 Al(l) 3 Mn(l) + 2 Al2O3(s) A) 15.8 g B) 38.2 g C) 47.4 g D) 50.9 g E) 67.8 g Section: 9.8 Limiting Reactant Problems 6) How many moles of oxygen react with 1.00 mol of butane, C4H10? C4H10(g) + O2(g) A) 1.00 mol B) 6.50 mol C) 13.0 mol D) 26.0 mol Section: General Exercises CO2(g) + H2O(g)

9 117) How many moles of oxygen gas react with 6.00 mol of propane, C3H8? C3H8(g) + O2(g) A) 3.00 mol B) 4.00 mol C) 5.00 mol D) 6.00 mol Answer: E Section: General Exercises CO2(g) + H2O(g) 118) How many moles of oxygen gas react with 6.00 mol of pentane, C5H12? C5H12(g) + O2(g) CO2(g) + H2O(g) A) 1.00 mol B) 5.00 mol C) 6.00 mol D) 8.00 mol Answer: E Section: General Exercises 119) How many moles of carbon dioxide are produced from 1.00 mol butane, C4H10? C4H10(g) + O2(g) A) 1.00 mol B) 4.00 mol C) 8.00 mol D) 16.0 mol Section: General Exercises CO2(g) + H2O(g)

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