CHEM Chapter 3 - Bimodal Questions

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

A

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

A

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

A

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

A

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

A

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

A

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)

A

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

A

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

A

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

A

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

A

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

A

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

A

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

A

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

A

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

A

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

A

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

A

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

A

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

A

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

A

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

B

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

B

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

B

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

B

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

B

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

B

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

B

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

B

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

B

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

B

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

B

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

B

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

B

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

B

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

B

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

B

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

B

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

C

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

C

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

C

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

C

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

C

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

C

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

C

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

C

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

C

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

C

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

C

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

C

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

C

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

C

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

C

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

C

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

D

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

D

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

D

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

D

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

D

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

D

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

D

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

D

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

D

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

D

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

D

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

D

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

E

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

E

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

E