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1 w ) if the expansion occurs against a constant pressure of 5.00 atm.A) -113 J B) 1.24 x 104 J C) -1.14 x 104 J D) 113 J E) 1.14 x 104 J 2 E for the process isA) -1300 cal B) 4700 cal C) 1300 cal D) -4700 cal E) 2350 cal 3 not a state function?A) ΔE B) ΔH C) q D) P E) V 4 H = ΔE ?A) 2HI(g ) → H2 (g ) + I2 (g ) at atmospheric pressure. B) Two moles of ammonia gas are cooled from 325 °C to 300 °C at 1.2 atm. C) H2 O(l ) → H2 O(g ) at 100 °C at atmospheric pressure. D) CaCO3 (s ) → CaO(s ) + CO2 (g ) at 800 °C at atmospheric pressure. E) CO2 (s ) → CO2 (g ) at atmospheric pressure. 5 2 (g ) + ½O2 (g ) → H2 O(g ) ΔH = -241.8 kJ2 (g ) + ½O2 (g ) → H2 O(l ) ΔH = -285.8 kJfalse ?A) Reaction (1) is exothermic. B) Reaction (2) is the formation reaction for H2 O(l ). C) The reverse of reaction (2) is endothermic. D) The energy content of H2 O(g ) is lower than H2 O(l ). E) ΔH for the reaction: H2 O(l ) → H2 O(g ) is + 44 kJ/mol. 6 A) 3.0 x 103 kJ B) 36 J C) 2.5 x 103 kJ D) 2.5 x 106 kJ E) 25 kJ 7 M HCl at 22.00 °C is added to 50. mL (50. g) of 1.00 M NaOH at 22.00 °C in a coffee cup calorimeter, the temperature increases to 28.87 °C. What is the heat (q ) of the reaction between HCl and NaOH? (The specific heat of the solution produced is 4.18 J/g·°C.)A) -6.3 x 103 J B) -3.2 x 103 J C) -2.9 x 103 J D) -1.7 x 103 J E) -1.4 x 103 J 8 A) 13.3 kJ B) 20.5 kJ C) 46.0 kJ D) 86.8 kJ E) none of the above 9 2 (g ) + ½O2 (g ) → SO3 (g ) ΔH ° = -99kJ 3 (g ) → O2 (g ) + 2SO2 (g ) ΔH ° = ?A) 99 kJ B) -198 kJ C) 49.5 kJ D) -99 kJ E) 198 kJ 10 2 (g ) + ½O2 (g ) → SO3 (g ) ΔH = -99.1 kJH when 89.6 g of SO2 is converted to SO3 .A) -69.3 kJ B) -139 kJ C) 69.3 kJ D) 139 kJ E) -111 kJ 11 graphite ) + O2 (g ) → CO2 (g ) ΔH ° = -393.5 kJ2 (g ) + ½O2 (g ) → H2 O(l ) ΔH ° = -285.8 kJ 3 OH(l ) + 3/2O2 (g ) → CO2 (g ) + 2H2 O(l ) ΔH ° = -726.4 kJgraphite ) + 2H2 (g ) + ½O2 (g ) → CH3 OH(l )A) +238.7 kJ B) -238.7 kJ C) +548.3 kJ D) -548.3 kJ E) +904.5 kJ 12 s ) + O2 (g ) → 2BaO(s ) ΔH ° = -1107.0 kJ 2 (g ) + ½O2 (g ) → BaCO3 (s ) ΔH ° = -822.5 kJ
H ° for the reaction below.3 (s ) → BaO(s ) + CO2 (g )A) -1929.5 kJ B) -1376.0 kJ C) -284.5 kJ D) 269.0 kJ E) 537 kJ 13 formation reaction of H2 SO4 (l )?A) H2 (g ) + S(s ) + 2O2 (g ) → H2 SO4 (l ) B) H2 SO4 (l ) → H2 (g ) + S(s ) + 2O2 (g ) C) H2 (g ) + S(g ) + 2O2 (g ) → H2 SO4 (l ) D) H2 SO4 (l ) → 2H(g) + S(s ) + 4O(g ) E) 2H(g) + S(g ) + 4O(g ) → H2 SO4 (l ) 14 H °f values: CH4 (g ), -74.8 kJ; CO2 (g ), -393.5 kJ; H2 O(l ), -285.8 kJ.H °f data above, calculate ΔH °rxn for the reaction below.4 (g ) + 2O2 (g ) → CO2 (g ) + 2H2 O(l )A) -604.2 kJ B) 890.3 kJ C) -997.7 kJ D) -890.3 kJ E) none of the above
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