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Chapter 5: Q23E (page 270)
If a reaction produces 1.506 kJ of heat, which is trapped in 30.0 g of water initially at 26.5 °C in a calorimeter like that in Figure 5.12, what is the resulting temperature of the water?
The resulting final temperature of the water is 38.5 °C.
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Before the introduction of chlorofluorocarbons, sulfur dioxide (enthalpy of vaporization, 6.00 kcal/mol) was used in household refrigerators. What mass of \({\bf{S}}{{\bf{O}}_{\bf{2}}}\)must be evaporated to remove as much heat as evaporation of 1.00 kg of \({\bf{CC}}{{\bf{l}}_{\bf{2}}}{{\bf{F}}_{\bf{2}}}\) (enthalpy of vaporization is 17.4 kJ/mol)?
The vaporization reactions for \({\bf{S}}{{\bf{O}}_{\bf{2}}}\)and \({\bf{CC}}{{\bf{l}}_{\bf{2}}}{{\bf{F}}_{\bf{2}}}\)are\({\bf{S}}{{\bf{O}}_{\bf{2}}}{\bf{(l)}} \to {\bf{S}}{{\bf{O}}_{\bf{2}}}{\bf{(g) and CC}}{{\bf{l}}_{\bf{2}}}{\bf{F(l) }} \to {\bf{CC}}{{\bf{l}}_{\bf{2}}}{{\bf{F}}_{\bf{2}}}{\bf{(g)}}\), respectively.
A 70.0-g piece of metal at 80.0 °C is placed in 100 g of water at 22.0 °C contained in a calorimeter like that shown in Figure 5.12. The metal and water come to the same temperature at 24.6 °C. How much heat did the metal give up to the water? What is the specific heat of the metal?
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)
When 1.0g of fructose, C6H12O6(s), a sugar commonly found in fruits, is burned in oxygen in a bomb calorimeter, the temperature of the calorimeter increases by 1.58˚C. If the heat capacity of the contents is 9.90kJ/˚C, what is q for this combustion?
Question: An aluminum kettle weighs 1.05 kg.
(a) What is the heat capacity of the kettle?
(b) How much heat is required to increase the temperature of this kettle from 23.0 °C to 99.0 °C?
(c) How much heat is required to heat this kettle from 23.0 °C to 99.0 °C if it contains 1.25 L of water (density of 0.997 g/mL and specific heat of 4.184 J/g °C)?
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