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Chapter 5: Q5.3-49E (page 227)
When 2.50 g of methane burns in oxygen, 125 kJ of heat is produced. What is the enthalpy of combustion per mole of methane under these conditions?
Enthalpy of combustion per mole of methane under these conditions will be -800 kJ.
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When 100 mL of 0.200 M NaCl(aq) and 100 mL of 0.200 M AgNO3(aq), both at 21.9 掳C, are mixed in a coffee cup calorimeter, the temperature increases to 23.5 掳C as solid AgCl forms. How much heat is produced by this precipitation reaction? What assumptions did you make to determine your value?
The enthalpy of combustion of hard coal averages -35 kJ/g, that of gasoline, \({\bf{1}}{\bf{.28 \times 1}}{{\bf{0}}^{\bf{5}}}\)kJ/gal. How many kilograms of hard coal provide the same amount of heat as is available from 1.0 gallons of gasoline? Assume that the density of gasoline is 0.692 g/mL (the same as the density of isooctane).
If a reaction produces 1.506 kJ of heat, which is trapped in 30.0 g of water initially at 26.5 掳C in a calorimeter like that in Figure 5.12, what is the resulting temperature of the water?
Ethylene, \({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{2}}}\), a byproduct from the fractional distillation of petroleum, is fourth among the 50 chemical compounds produced commercially in the largest quantities. About 80% of synthetic ethanol is manufactured from ethylene by its reaction with water in the presence of a suitable catalyst. \({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{2}}}{\bf{(g) + }}{{\bf{H}}_{\bf{2}}}{\bf{O(g)}} \to {{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{5}}}{\bf{OH(l)}}\).Using the data in the table inAppendix G, calculate 螖H掳 for the reaction.
Water gas, a mixture of \({{\bf{H}}_{\bf{2}}}\) and CO, is an important industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon:\({\bf{C}}\left( {\bf{s}} \right){\bf{ + }}{{\bf{H}}_{\bf{2}}}{\bf{O}}\left( {\bf{g}} \right) \to {\bf{CO}}\left( {\bf{g}} \right){\bf{ + }}{{\bf{H}}_{\bf{2}}}\left( {\bf{g}} \right)\).
(a) Assuming that coke has the same enthalpy of formation as graphite, calculate \({\bf{\Delta H}}_{{\bf{298}}}^{\bf{0}}\)for this reaction.
(b) Methanol, a liquid fuel that could possibly replace gasoline, can be prepared from water gas and additional hydrogen at high temperature and pressure in the presence of a suitable catalyst:\({\bf{2}}{{\bf{H}}_{\bf{2}}}\left( {\bf{g}} \right){\bf{ + CO}}\left( {\bf{g}} \right) \to {\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{OH}}\left( {\bf{g}} \right)\).
Under the conditions of the reaction, methanol forms as a gas. Calculate \({\bf{\Delta H}}_{{\bf{298}}}^{\bf{0}}\)for this reaction and for the condensation of gaseous methanol to liquid methanol.
(c) Calculate the heat of combustion of 1 mole of liquid methanol to H2O(g) and CO2(g).
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