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Chapter 5: Q7E (page 268)
Question: How much heat, in joules and in calories, is required to heat a 28.4-g (1-oz) ice cube from 鈭�23.0 掳C to 鈭�1.0 掳C?
The heat required to raise the temperature in joules =130.77 J
The heat required to raise the temperature in calories =31.24 calories
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How many kilojoules of heat will be released when exactly 1 mole of iron, Fe, is burned to form Fe2O3(s) at standard state conditions?
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).
A 45-g aluminum spoon (specific heat 0.88 J/g 掳C) at 24掳C is placed in 180 mL (180 g) of coffee at 85掳C and the temperature of the two becomes equal.
(a) What is the final temperature when the two become equal? Assume that coffee has the same specific heat as water.
(b) The first time a student solved this problem she got an answer of 88 掳C. Explain why this is clearly an incorrect answer.
Assume that the coffee has the same density and specific heat as water.
In the early days of automobiles, illumination at night was provided by burning acetylene, C2H2. Though no longer used as auto headlamps, acetylene is still used as a source of light by some cave explorers. The acetylene is (was) prepared in the lamp by the reaction of water with calcium carbide, CaC2:
\({\bf{Ca}}{{\bf{C}}_{\bf{2}}}\left( {\bf{s}} \right){\bf{ + 2}}{{\bf{H}}_{\bf{2}}}{\bf{O}}\left( {\bf{l}} \right) \to {\bf{Ca}}{\left( {{\bf{OH}}} \right)_{\bf{2}}}\left( {\bf{s}} \right){\bf{ + }}{{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{2}}}\left( {\bf{g}} \right)\)
Calculate the standard enthalpy of the reaction. The \({\bf{\Delta H}}_{\bf{f}}^{\bf{o}}\)of CaC2is -15.14 kcal/mol.
What mass of carbon monoxide must be burned to produce 175 kJ of heat under standard state conditions?
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