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27) The value of ΔH° for the reaction below is -1107 kJ:
2Ba (s) + O2 (g) → 2BaO (s)
How many kJ of heat are released when 5.75 g of Ba (s) reacts completely with oxygen to form BaO (s)?
A) 96.3 kJ
B) 26.3 kJ
C) 46.4 kJ
D) 23.2 kJ
E) 193 kJ
28) The value of ΔH° for the reaction below is -1107 kJ:
2Ba (s) + O2 (g) → 2BaO (s)
How many kJ of heat are released when 5.75 g of BaO (s) is produced?
A) 56.9 kJ
B) 23.2 kJ
C) 20.8 kJ
D) 193 kJ
E) 96.3 kJ
29) The value of ΔH° for the reaction below is -1107 kJ:
2Ba (s) + O2 (g) → 2BaO (s)
How many kJ of heat are released when 15.75 g of Ba (s) reacts completely with oxygen to form BaO (s)?
A) 20.8 kJ
B) 63.5 kJ
C) 114 kJ
D) 70.3 kJ
E) 35.1 kJ
30) The molar heat capacity of a compound with the formula C2H6 SO is 88.0 J/mol-K. The specific heat
of this substance is ________ J/g-K.
A) 88.0
B) 1.13
C) 4.89
D) 6.88 × 103
E) -88.0
31) The specific heat capacity of lead is 0.13 J/g-K. How much heat (in J) is required to raise the
temperature of 15 g of lead from 22 °C to 37 °C?
A) 2.0 J
B) -0.13 J
C) 5.8 × 10-4 J
D) 29 J
E) 0.13 J
32) The temperature of a 15-g sample of lead metal increases from 22 °C to 37 °C upon the addition of 29.0
J of heat. The specific heat capacity of the lead is ________ J/g-K.
A) 7.8
B) 1.9
C) 29
D) 0.13
E) -29
33) The specific heat of bromine liquid is 0.226 J/g-K. The molar heat capacity (in J/mol-K) of bromine
liquid is ________.
A) 707 J/mol-K
B) 36.1 J/mol-K
C) 18.1 J/mol-K
D) 9.05 J/mol-K
E) 0.226 J/mol-K
34) The specific heat of liquid bromine is 0.226 J/g-K. How much heat (J) is required to raise the
temperature of 10.0 mL of bromine from 25.00 °C to 27.30 °C? The density of liquid bromine: 3.12 g/mL.
A) 5.20 J
B) 16.2 J
C) 300 J
D) 32.4 J
E) 10.4 J
35) ΔH for the reaction
IF5 (g) → IF3 (g) + F2 (g)
is ________ kJ, give the data below.
IF (g) + F2 (g) → IF3 (g) ΔH = -390 kJ
IF (g) + 2F2 (g) → IF5 (g) ΔH = -745 kJ
A) +355
B) -1135
C) +1135
D) +35
E) -35
36) Given the following reactions
Fe2O3 (s) + 3CO (s) → 2Fe (s) + 3CO2 (g) ΔH = -28.0 kJ
3Fe (s) + 4CO2 (s) → 4CO (g) + Fe3O4 (s) ΔH = +12.5 kJ
the enthalpy of the reaction of Fe2O3 with CO
3Fe2O3 (s) + CO (g) → CO2 (g) + 2 Fe3O4 (s)
is ________ kJ.
A) -59.0
B) 40.5
C) -15.5
D) -109
E) +109
37) Given the following reactions
N2 (g) + 2O2 (g) → 2NO2 (g) ΔH = 66.4 kJ
2NO (g) + O2 (g) → 2NO2 (g) ΔH = -114.2 kJ
the enthalpy of the reaction of the nitrogen to produce nitric oxide
N2 (g) + O2 (g) → 2NO (g)
is ________ kJ.
A) 180.6
B) -47.8
C) 47.8
D) 90.3
E) -180.6
38) Given the following reactions
2NO → N2 + O2 ΔH = -180 kJ
2NO + O2 → 2NO2 ΔH = -112 kJ
the enthalpy of the reaction of nitrogen with oxygen to produce nitrogen dioxide
N2 + 2O2 → 2NO2
is ________ kJ.
A) 68
B) -68
C) -292
D) 292
E) -146
39) Given the following reactions
2S (s) + 3O2 (g) → 2SO3 (g) ΔH = -790 kJ
S (s) + O2 (g) → SO2 (g) ΔH = -297 kJ
the enthalpy of the reaction in which sulfur dioxide is oxidized to sulfur trioxide
2SO2 (g) + O2 (g) → 2SO3 (g)
is ________ kJ.
A) 196
B) -196
C) 1087
D) -1384
E) -543
40) Given the following reactions
CaCO3 (s) → CaO (s) + CO2 (g) ΔH = 178.1 kJ
C (s, graphite) + O2 (g) → CO2 (g) ΔH = -393.5 kJ
the enthalpy of the reaction
CaCO3 (s) → CaO (s) + C (s, graphite) + O2 (g)
is ________ kJ.
A) 215.4
B) 571.6
C) -215.4
D) -571.6
E) 7.01 × 104
41) Given the following reactions
H2O (l) → H2O (g) ΔH = 44.01 kJ
2H2 (g) + O2 (g) → 2H2O (g) ΔH = -483.64 kJ
the enthalpy for the decomposition of liquid water into gaseous hydrogen and oxygen
2H2O (l) → 2H2 (g) + O2 (g)
is ________ kJ.
A) -395.62
B) -527.65
C) 439.63
D) 571.66
E) 527.65
42) Given the following reactions
N2 (g) + O2 (g) → 2NO (g) ΔH = +180.7 kJ
2NO( g) + O2 (g) → 2NO2 (g) ΔH = -113.1 kJ
the enthalpy for the decomposition of nitrogen dioxide into molecular nitrogen and oxygen
2NO2 (g) → N2 (g) + 2O2 (g)
is ________ kJ.
A) 67.6
B) -67.6
C) 293.8
D) -293.8
E) 45.5
43) Given the following reactions
N2 (g) + O2 (g) → 2NO (g) ΔH = +180.7 kJ
2NO (g) + O2 (g) → 2NO2 (g) ΔH = -113.1 kJ
the enthalpy of reaction for
4NO (g) → 2NO2 (g) + N2 (g)
is ________ kJ.
A) 67.6
B) 45.5
C) -293.8
D) -45.5
E) 293.8
44) Given the following reactions
N2 (g) + O2 (g) → 2NO (g) ΔH = +180.7 kJ
2N2O (g) → O2 (g) + 2N2 (g) ΔH = -163.2 kJ
the enthalpy of reaction for
2N2O (g) → 2NO (g) + N2 (g)
is ________ kJ.
A) 145.7
B) 343.9
C) -343.9
D) 17.5
E) -145.7
45) The value of ΔH° for the reaction below is -186 kJ.
H2 (g) + Cl2 (g) → 2HCl (g)
The value of ΔH°f for HCl (g) is ________ kJ/mol.
A) -3.72 × 102
B) -1.27 × 102
C) -93.0
D) -186
E) +186
46) The value of ΔH° for the following reaction is -3351 kJ:
2Al (s) + 3O2 (g) → 2Al2O3 (s)
The value of ΔH°f for Al2O3 (s) is ________ kJ.
A) -3351
B) -1676
C) -32.86
D) -16.43
E) +3351
47) Given the data in the table below, ΔH°rxn for the reaction
Ca(OH)2 + 2H3AsO4 → Ca(H2AsO4)2 + 2H2O
is ________ kJ.
A) -744.9
B) -4519
C) -4219
D) -130.4
E) -76.4
48) Given the data in the table below, ΔH°rxn for the reaction
4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (l)
is ________ kJ.
A) -1172
B) -150
C) -1540
D) -1892
E) The ΔH°f of O2 (g) is needed for the calculation.
49) Given the data in the table below, ΔH°rxn for the reaction
C2H5OH (l) + O2 (g) → CH3CO2H (l) + H2O (l)
is ________ kJ.
A) -79.0
B) -1048.0
C) -476.4
D) -492.6
E) The value of ΔH°f of O2 (g) is required for the calculation.
50) Given the data in the table below, ΔH°rxn for the reaction
3NO2 (g) + H2O (l) → 2HNO3 (aq) + NO (g)
is ________ kJ.
A) 64
B) 140
C) -140
D) -508
E) -64
51) Given the data in the table below, ΔH°rxn for the reaction
IF5 (g) + F2 (g) → IF7 (g)
is ________ kJ.
A) 1801
B) -1801
C) 121
D) -121
E) -101
52) Given the data in the table below, ΔH° for the reaction
2CO (g) + O2 (g) → 2CO2 (g)
is ________ kJ.
A) -566.4
B) -283.2
C) 283.2
D) -677.0
E) The ΔH°f of O2 (g) is needed for the calculation.
53) The value of ΔH° for the following reaction is 177.8 kJ. The value of ΔH°f for CaO(s) is ________
kJ/mol.
CaCO3 (s) → CaO (s) + CO2 (g)
A) -1600
B) -813.4
C) -635.5
D) 813.4
E) 177.8
54) Given the data in the table below, ΔH°rxn for the reaction
2Ag2S (s) + O2 (g) → 2Ag2O (s) + 2S (s)
is ________ kJ.
A) -1.6
B) +1.6
C) -3.2
D) +3.2
E) The ΔH°f of S (s) and of O2 (g) are needed for the calculation.
55) Given the data in the table below, ΔH°rxn for the reaction
Ag2O (s) + H2S (g) → Ag2S (s) + H2O (l)
is ________ kJ.
A) -267
B) -370
C) -202
D) -308
E) More data are needed to complete the calculation.
56) Given the data in the table below, ΔH°rxn for the reaction
2SO2 (g) + O2 (g) → 2SO3 (g)
is ________ kJ.
A) -99
B) 99
C) -198
D) 198
E) The ΔH°f of O2 (g) is needed for the calculation.
57) Given the data in the table below, ΔH°rxn for the reaction
SO3 (g) + H2O (l) → H2SO4 (l)
is ________ kJ.
A) -132
B) 1496
C) 704
D) -704
E) -2.16 × 103
58) Given the data in the table below, ΔH°rxn for the reaction
3 Cl2 (g) + PH3 (g) → PCl3 (g) + 3 HCl (g)
is ________ kJ.
A) -385.77
B) -570.37
C) 570.37
D) 385.77
E) The ΔH°f of Cl2 (g) is needed for the calculation.
59) Given the data in the table below, ΔH°rxn for the reaction
PCl3 (g) + 3 HCl (g) → 3Cl2 (g) + PH3 (g)
is ________ kJ.
A) -570.37
B) -385.77
C) 570.37
D) 385.77
E) The ΔH°f of Cl2 (g) is needed for the calculation.
