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Chapter 5: Q45E (page 227)
How much heat is produced by burning 4.00 moles of acetylene under standard conditions?
The heat produced by burning 4 mol of acetylene under standard conditions is 5204.4 kJ.
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From the molar heats of formation in Appendix G, determine how much heat is required to evaporate one mole of water:\({{\bf{H}}_{\bf{2}}}{\bf{O}}\left( {\bf{l}} \right) \to {{\bf{H}}_{\bf{2}}}{\bf{O}}\left( {\bf{g}} \right)\)
When a 3.00-g sample of KCl was added to 3.00×102 g of water in a coffee cup calorimeter, the temperature decreased by 1.05 °C. How much heat is involved in the dissolution of the KCl? What assumptions did you make?
When 1.42 g of iron reacts with 1.80 g of chlorine, 3.22 g of \({\bf{FeC}}{{\bf{l}}_{\bf{2}}}\)(s) and 8.60 kJ of heat is produced. What is the enthalpy change for the reaction when 1 mole of \({\bf{FeC}}{{\bf{l}}_{\bf{2}}}\)(s) is produced?
The addition of 3.15g of Ba(OH)2.8H2O to a solution of 1.52g of NH4SCN in 100g of water in a calorimeter caused the temperature to fall by 3.1˚C. Assuming the specific heat of the solution and products is 4.20J/g˚C, calculate the approximate amount of heat absorbed by the reaction, which can be represented by the following equation:
Ba(OH)2.8H2O(s) + 2NH4SCN (aq) -------> Ba(SCN)2(aq) + 2NH3(aq) + 10H2O(l)
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 ΔH° for the reaction.
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