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CHEM Chapter 3 - Bimodal Questions

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10) When the following equation is balanced, the coefficient of H3PO4 is ________. H3PO4 (aq) + NaOH (aq) → Na3PO4 (aq) + H2O (l) A) 1 B) 2 C) 3 D) 4 E) 0

14) When the following equation is balanced, the coefficient of H2SO4 is ________. H2SO4 (aq) + NaOH (aq) → Na2SO4 (aq) + H2O (l) A) 1 B) 2 C) 3 D) 4 E) 0.5

16) When the following equation is balanced, the coefficient of hydrogen is ________. K (s) + H2O (l) → KOH (aq) + H2 (g) A) 1 B) 2 C) 3 D) 4 E) 5

19) When the following equation is balanced, the coefficient of dinitrogen pentoxide is ________. N2O5 (g) + H2O (l) → HNO3 (aq) A) 1 B) 2 C) 3 D) 4 E) 5

2) When the following equation is balanced, the coefficients are ________. Al(NO3)3 + Na2S → Al2S3 + NaNO3 A) 2, 3, 1, 6 B) 2, 1, 3, 2 C) 1, 1, 1, 1 D) 4, 6, 3, 2 E) 2, 3, 2, 3

25) Predict the product in the combination reaction below. Al (s) + N2 (g) → ________ A) AlN B) Al3N C) AlN2 D) Al3N2 E) AlN3

26) The balanced equation for the decomposition of sodium azide is ________. A) 2NaN3 (s) → 2Na (s) + 3N2 (g) B) 2NaN3 (s) → Na2 (s) + 3N2 (g) C) NaN3 (s) → Na (s) + N2 (g) D) NaN3 (s) → Na (s) + N2 (g) + N (g) E) 2NaN3 (s) → 2Na (s) + 2N2 (g)

3) When the following equation is balanced, the coefficient of H2 is ________. K (s) + H2O (l) → KOH (aq) + H2 (g) A) 1 B) 2 C) 3 D) 4 E) 5

30) A sample of C3H8O that contains 200 molecules contains ________ carbon atoms. A) 600 B) 200 C) 3.61 × 1026 D) 1.20 × 1026 E) 4.01 × 1025

35) What is the empirical formula of a compound that contains 29% Na, 41% S, and 30% O by mass? A) Na2S2O3 B) NaSO2 C) NaSO D) NaSO3 E) Na2S2O6

37) A compound contains 40.0% C, 6.71% H, and 53.29% O by mass. The molecular weight of the compound is 60.05 amu. The molecular formula of this compound is ________. A) C2H4O2 B) CH2O C) C2H3O4 D) C2H2O4 E) CHO2

38) A compound that is composed of carbon, hydrogen, and oxygen contains 70.6% C, 5.9% H, and 23.5% O by mass. The molecular weight of the compound is 136 amu. What is the molecular formula? A) C8H8O2 B) C8H4O C) C4H4O D) C9H12O E) C5H6O2

39) A compound that is composed of only carbon and hydrogen contains 85.7% C and 14.3% H by mass. What is the empirical formula of the compound? A) CH2 B) C2H4 C) CH4 D) C4H8 E) C86H14

41) A compound contains 38.7% K, 13.9% N, and 47.4% O by mass. What is the empirical formula of the compound? A) KNO3 B) K2N2O3 C) KNO2 D) K2NO3 E) K4NO5

43) Combustion of a 1.031-g sample of a compound containing only carbon, hydrogen, and oxygen produced 2.265 g of CO2 and 1.236 g of H2O. What is the empirical formula of the compound? A) C3H8O B) C3H5O C) C6H16O2 D) C3H9O3 E) C3H6O3

46) The combustion of propane (C3H8) in the presence of excess oxygen yields CO2 and H2O: C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g) When 2.5 mol of O2 are consumed in their reaction, ________ mol of CO2 are produced. A) 1.5 B) 3.0 C) 5.0 D) 6.0 E) 2.5

57) What mass in grams of hydrogen is produced by the reaction of 4.73 g of magnesium with 1.83 g of water? Mg (s) + 2H2O (l) → Mg(OH)2 (s) + H2 (g) A) 0.102 B) 0.0162 C) 0.0485 D) 0.219 E) 0.204

58) If the reaction yield is 94.4%, what mass in grams of hydrogen is produced by the reaction of 4.73 g of magnesium with 1.83 g of water? Mg (s) + 2H2O (l) → Mg(OH)2 (s) + H2 (g) A) 0.0962 B) 0.0162 C) 0.0485 D) 0.219 E) 0.204

6) When the following equation is balanced, the coefficient of Al2O3 is ________. Al2O3 (s) + C (s) + Cl2 (g) → AlCl3 (s) + CO (g) A) 1 B) 2 C) 3 D) 4 E) 5

60) How many moles of magnesium oxide are produced by the reaction of 3.82 g of magnesium nitride with 7.73 g of water? Mg3N2 + 3H2O → 2NH3 + 3MgO A) 0.114 B) 0.0378 C) 0.429 D) 0.0756 E) 4.57

67) Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O2 (g) → 2Al2O3 (s) In a particular experiment, the reaction of 2.5 g of Al with 2.5 g of O2 produced 3.5 g of Al2O3. The % yield of the reaction is ________. A) 74 B) 37 C) 47 D) 66 E) 26

1) When the following equation is balanced, the coefficients are ________. NH3 (g) + O2 (g) → NO2 (g) + H2O (g) A) 1, 1, 1, 1 B) 4, 7, 4, 6 C) 2, 3, 2, 3 D) 1, 3, 1, 2 E) 4, 3, 4, 3

11) When the following equation is balanced, the coefficient of C3H8O3 is ________. C3H8O3 (g) + O2 (g) → CO2 (g) + H2O (g) A) 1 B) 2 C) 3 D) 7 E) 5

15) When the following equation is balanced, the coefficient of water is ________. K (s) + H2O (l) → KOH (aq) + H2 (g) A) 1 B) 2 C) 3 D) 4 E) 5

17) When the following equation is balanced, the coefficient of oxygen is ________. PbS (s) + O2 (g) → PbO (s) + SO2 (g) A) 1 B) 3 C) 2 D) 4 E) 5

21) When the following equation is balanced, the coefficient of nitric acid is ________. N2O5 (g) + H2O (l) → HNO3 (aq) A) 5 B) 2 C) 3 D) 4 E) 1

22) Write the balanced equation for the reaction that occurs when methanol, CH3OH (l), is burned in air. What is the coefficient of methanol in the balanced equation? A) 1 B) 2 C) 3 D) 4 E) 3/2

31) How many moles of carbon monoxide are there in 36.55 g of carbon monoxide? A) 0.8452 B) 1.305 C) 0.9291 D) 2.589 E) 3.046

32) How many moles of carbon dioxide are there in 52.06 g of carbon dioxide? A) 0.8452 B) 1.183 C) 6.022 × 1023 D) 8.648 × 1023 E) 3.134 × 1025

34) What is the empirical formula of a compound that contains 27.0% S, 13.4% O, and 59.6% Cl by mass? A) SOCl B) SOCl2 C) S2OCl D) SO2Cl E) ClSO4

4) When the following equation is balanced, the coefficient of Al is ________. Al (s) + H2O (l) → Al(OH)3 (s) + H2 (g) A) 1 B) 2 C) 3 D) 5 E) 4

42) A compound is composed of only C, H, and O. The combustion of a 0.519-g sample of the compound yields 1.24 g of CO2 and 0.255 g of H2O. What is the empirical formula of the compound? A) C6H6O B) C3H3O C) CH3O D) C2H6O5 E) C2H6O2

5) When the following equation is balanced, the coefficient of H2O is ________. Ca (s) + H2O (l) → Ca(OH)2 (aq) + H2 (g) A) 1 B) 2 C) 3 D) 5 E) 4

61) A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water: Mg3N2 + 3H2O → 2NH3 + 3MgO The yield of MgO is 3.60 g. What is the percent yield in the reaction? A) 94.5 B) 78.4 C) 46.6 D) 49.4 E) 99.9

63) What is the maximum mass in grams of NH3 that can be produced by the reaction of 1.0 g of N2 with 3.0 g of H2 via the equation below? N2 (g) + H2 (g) → NH3 (g) (not balanced) A) 2.0 B) 1.2 C) 0.61 D) 17 E) 4.0

64) What is the maximum amount in grams of SO3 that can be produced by the reaction of 1.0 g of S with of O2 via the equation below? S (s) + O2 (g) → SO3 (g) (not balanced) A) 0.27 B) 1.7 C) 2.5 D) 3.8 E) 2.0

8) When the following equation is balanced, the coefficient of HCl is ________. CaCO3 (s) + HCl (aq) → CaCl2 (aq) + CO2 (g) + H2O (l) A) 1 B) 2 C) 3 D) 4 E) 0

9) When the following equation is balanced, the coefficient of HNO3 is ________. HNO3 (aq) + CaCO3 (s) → Ca(NO3)2 (aq) + CO2 (g) + H2O (l) A) 1 B) 2 C) 3 D) 5 E) 4

13) When the following equation is balanced, the coefficient of H2 is ________. CO (g) + H2 (g) → H2O (g) + CH4 (g) A) 1 B) 2 C) 3 D) 4 E) 0

23) Write the balanced equation for the reaction that occurs when methanol, CH3OH (l), is burned in air. What is the coefficient of oxygen in the balanced equation? A) 1 B) 2 C) 3 D) 4 E) 3/2

24) What is the coefficient of O2 when the following equation is completed and balanced? C4H8O2 + O2 → ________ A) 2 B) 3 C) 5 D) 6 E) 1

27) There are ________ mol of carbon atoms in 4 mol of C4H8O2. A) 4 B) 8 C) 16 D) 20 E) 32

40) A compound that is composed of only carbon and hydrogen contains 80.0% C and 20.0% H by mass. What is the empirical formula of the compound? A) C20H60 B) C7H20 C) CH3 D) C2H6 E) CH4

44) Combustion of a 0.9827-g sample of a compound containing only carbon, hydrogen, and oxygen produced 1.900 g of CO2 and 1.070 g of H2O. What is the empirical formula of the compound? A) C2H5O B) C4H10O2 C) C4H11O2 D) C4H10O E) C2H5O2

45) The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O: 4 NH3 (g) + 7 O2 (g) → 4 NO2 (g) + 6 H2O (g) The combustion of 43.9 g of ammonia produces ________ g of NO2. A) 2.58 B) 178 C) 119 D) 0.954 E) 43.9

47) Calcium carbide (CaC2) reacts with water to produce acetylene (C2H2): CaC2 (s) + 2H2O (g) → Ca(OH)2 (s) + C2H2 (g) Production of 13 g of C2H2 requires consumption of ________ g of H2O. A) 4.5 B) 9.0 C) 18 D) 4.8 × 102 E) 4.8 × 10-2

48) Calcium carbide (CaC2) reacts with water to produce acetylene (C2H2): CaC2 (s) + 2H2O (g) → Ca(OH)2 (s) + C2H2 (g) The complete reaction of 57.4 g of CaC2 requires consumption of ________ g of H2O. A) 0.895 B) 64.1 C) 32.3 D) 1.79 E) 18.0

53) GeF3H is formed from GeH4 and GeF4 in the combination reaction: GeH4 + 3GeF4 → 4GeF3H If the reaction yield is 92.6%, how many moles of GeF4 are needed to produce 8.00 mol of GeF3H? A) 3.24 B) 5.56 C) 6.48 D) 2.78 E) 2.16

55) Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: PbCO3 (s) → PbO (s) + CO2 (g) If the reaction yield is 95.7%, how many grams of lead (II) oxide will be produced by the decomposition of 2.50 g of lead (II) carbonate? A) 1.04 B) 1.55 C) 2.18 D) 4.00 E) 5.55

56) The combustion of ammonia in the presence of oxygen yields NO2 and H2O: 4 NH3 (g) + 7O2 (g) → 4 NO2 (g) + 6 H2O (g) The combustion of 43.9 g of ammonia with 258 g of oxygen produces ________ g of NO2. A) 212 B) 178 C) 119 D) 0.954 E) 43.9

65) Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O2 (g) → 2Al2O3 (s) The maximum amount of Al2O3 that can be produced from 2.5 g of Al and 2.5 g of O2 is ________ g. A) 9.4 B) 7.4 C) 4.7 D) 5.3 E) 5.0

66) Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s) + 3F2 (g) → SF6 (g) The maximum amount of SF6 that can be produced from the reaction of 3.5 g of sulfur with 4.5 g of fluorine is ________ g. A) 12 B) 3.2 C) 5.8 D) 16 E) 8.0

69) Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s) + 3F2 (g) → SF6 (g) In a particular experiment, the percent yield is 79.0%. This means that in this experiment, a 7.90-g sample of fluorine yields ________ g of SF6. A) 30.3 B) 10.1 C) 7.99 D) 24.0 E) 0.110

7) When the following equation is balanced, the coefficient of H2S is ________. FeCl3 (aq) + H2S (g) → Fe2S3 (s) + HCl (aq) A) 1 B) 2 C) 3 D) 5 E) 4

12) When the following equation is balanced, the coefficient of O2 is ________. C2H4O (g) + O2 (g) → CO2 (g) + H2O (g) A) 2 B) 3 C) 4 D) 5 E) 1

18) When the following equation is balanced, the coefficient of sulfur dioxide is ________. PbS (s) + O2 (g) → PbO (s) + SO2 (g) A) 5 B) 1 C) 3 D) 2 E) 4

28) There are ________ sulfur atoms in 25 molecules of C4H4S2. A) 1.5 × 1025 B) 4.8 × 1025 C) 3.0 × 1025 D) 50 E) 6.02 × 1023

29) There are ________ hydrogen atoms in 25 molecules of C4H4S2. A) 25 B) 3.8 × 1024 C) 6.0 × 1025 D) 100 E) 1.5 × 1025

33) There are ________ molecules of methane in 0.123 mol of methane (CH4). A) 5 B) 2.46 × 10-2 C) 2.04 × 10-25 D) 7.40 × 1022 E) 0.615

36) What is the empirical formula of a compound that contains 49.4% K, 20.3% S, and 30.3% O by mass? A) KSO2 B) KSO3 C) K2SO4 D) K2SO3 E) KSO4

49) Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N2 (g) + 3H2 (g) → 2NH3 (g) A 7.1-g sample of N2 requires ________ g of H2 for complete reaction. A) 0.51 B) 0.76 C) 1.2 D) 1.5 E) 17.2

50) Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N2 (g) + 3H2 (g) → 2NH3 (g) A ________ g sample of N2 requires 3.0 g of H2 for complete reaction. A) 0.51 B) 0.76 C) 1.2 D) 14.0 E) 17.2

51) Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: PbCO3 (s) → PbO (s) + CO2 (g) How many grams of lead (II) oxide will be produced by the decomposition of 2.50 g of lead (II) carbonate? A) 0.41 B) 2.50 C) 0.00936 D) 2.09 E) 2.61

52) The combustion of propane (C3H8) produces CO2 and H2O: C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g) The reaction of 2.5 mol of O2 with 4.6 mol of C3H8 will produce ________ mol of H2O. A) 4.0 B) 3.0 C) 2.5 D) 2.0 E) 1.0

54) Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N2 (g) + 3H2 (g) → 2NH3 (g) If the reaction yield is 87.5%, how many moles of N2 are needed to produce 3.00 mol of NH3? A) 0.166 B) 1.00 C) 1.5 D) 1.71 E) 2.32

59) Silver nitrate and aluminum chloride react with each other by exchanging anions: 3AgNO3 (aq) + AlCl3 (aq) → Al(NO3)3 (aq) + 3AgCl (s) What mass in grams of AgCl is produced when 4.22 g of AgNO3 react with 7.73 g of AlCl3? A) 17.6 B) 4.22 C) 24.9 D) 3.56 E) 11.9

20) When the following equation is balanced, the coefficient of water is ________. N2O5 (g) + H2O (l) → HNO3 (aq) A) 5 B) 2 C) 3 D) 4 E) 1

62) Pentacarbonyliron (Fe(CO)5) reacts with phosphorous trifluoride (PF3) and hydrogen, releasing carbon monoxide: Fe(CO)5 + PF3 + H2 → Fe(CO)2(PF3)2(H)2 + CO (not balanced) The reaction of 5.0 mol of Fe(CO)5 , 8.0 mol of PF3 and 6.0 mol of H2 will release ________ mol of CO. A) 15 B) 5.0 C) 24 D) 6.0 E) 12

68) Sulfur and oxygen react in a combination reaction to produce sulfur trioxide, an environmental pollutant: 2S (s) + 3O2 (g) → 2SO3 (g) In a particular experiment, the reaction of 1.0 g S with 1.0 g O2 produced 0.80 g of SO3. The % yield in this experiment is ________. A) 30 B) 29 C) 21 D) 88 E) 47

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