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1 w ) for this process.A) 2.8 x 104 J B) 1.0 x 104 J C) -2.8 x 102 J D) -2.8 x 104 J E) 2.8 x 102 J 2 E for the process isA) -555 J B) 750 J C) 555 J D) -195 J E) 195 J 3 q , w , and ΔE respectively?A) 128 J, 6.9 J, 135 J B) 128 J, -6.9 J, 121 J C) 128 J, 697 J, 825 J D) 128 J, -697 J, -569 J E) -128 J, -6.9 J, -135 J 4 A) ΔE = 0 B) ΔH = 0 C) ΔE < 0 D) w = 0E) q = 05 A) H2 (l ) → H2 (g ) B) CO2 (s ) → CO2 (g ) C) H2 O(g ) → H2 O(l ) D) 16CO2 (g ) + 18H2 O(l ) → 2C8 H18 (l ) + 25O2 (g ) E) H2 (g ) → 2H(g ) 6 A) the C-O and O-H single bonds in carbohydrates are weak. B) carbohydrates contain C-O and O-H bonds and hydrocarbons do not. C) the total energy of the C-C and C-H bonds in hydrocarbons is greater than the total energy of the C=O and O-H bonds in the combustion products (carbon dioxide and water). D) the total energy of the bonds in hydrocarbons is greater than the energy of the bonds in carbohydrates. E) hydrocarbons have higher molar masses than carbohydrates. 7 A) 208 J B) 9.5 J C) 60.1 J D) 1.49 x 103 J E) 1.70 x 103 J 8 2 CN(s ), with oxygen was run in a bomb calorimeter, and ΔE was found to be -742.7 kJ/mol of NH2 CN(s ) at 298 K. Calculate ΔH for the reaction at this temperature. 2 CN(s ) + 3/2O2 (g ) → N2 (g ) + CO2 (g ) + H2 O(l )A) -727.8 kJ/mol B) -737.7 kJ C) -741.5 kJ D) -742.7 kJ E) none of the above 9 3 OH) was burned in a constant-volume bomb calorimeter. Consequently the temperature of the water rose from 20.27 °C to 26.87 °C. If the mass of water surrounding the calorimeter was exactly 1000 g and the heat capacity of the bomb calorimeter was 1.75 kJ/°C, calculate the molar heat of combustion of liquid methanol .A) -8.17 x 105 kJ/mol B) -817 kJ/mol C) 1.88 kJ/mol D) -0.8 kJ/mol E) none of the above 10 s ) + O2 (g ) → CO2 (g ) ΔH °rxn = -393 kJs ) must burn in this way to release 275 kJ of heat?A) 0.70 g B) 1.43 g C) 8.40 g D) 17.1 g E) 275 g 11 2 H6 (g ), at constant pressure releases 259 kJ of heat. H for the reaction: 2C2 H6 (g ) + 7O2 (g ) → 4CO2 (g ) + 6H2 O(l )?A) -259 kJ B) -518 kJ C) -1295 kJ D) -1554 kJ E) -3108 kJ 12 2 H4 (g ) + 3O2 (g ) → 2CO2 (g ) + 2H2 O(l ) ΔH °f = -1411 kJ
s ) + O2 (g ) → CO2 (g ) ΔH °f = -393.5 kJ
2 (g ) + ½O2 (g ) → H2 O(l ) ΔH °f = -285.8 kJ 2 H4 (g ).A) 731 kJ/mol B) 87 kJ/mol C) 1.41 x 103 kJ/mol D) 52 kJ/mol E) 2.77 x 103 kJ/mol 13 s ) + O2 (g ) → 2FeO(s ) ΔH ° = -544.0 kJ s ) + 3O2 (g ) → 2Fe2 O3 (s ) ΔH ° = -1648.4 kJ 3 O4 (s ) → 3Fe(s ) + 2O2 (g ) ΔH ° = +1118.4 kJ H °, for the reaction below:2 O3 (s ) + FeO(s ) → Fe3 O4 (s )A) -1074.0 kJ B) -22.2 kJ C) +22.2 kJ D) +249.8 kJ E) +1074.0 kJ 14 not have a ΔH °f of zero under standard state conditions?A) H2 (g ) B) Li(s ) C) C (graphite ) D) Br2 (l ) E) O3 (g ) 15 8 H18 (l ) + 25O2 (g ) → 16CO2 (g ) + 18H2 O(l ) ΔH ° = -11,200. kJ H °f : 2 (g ), -393.5 kJ/mol; H2 O(l ), -285.8 kJ/molformation of octane, C8 H18 (l ).A) -120. kJ/mol B) -240. kJ/mol C) -5144 kJ/mol D) -6296 kJ/mol E) -11,440. kJ/mol
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