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Chapter 5: Q5.3-78E (page 274)
From the data in Table 5.2, determine which of the following fuels produces the greatest amount of heat per gram when burned under standard conditions: CO(g), CH4(g), or C2H2(g).
The greatest amount of heat per gram is produced by CO(g).
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Propane, \({{\bf{C}}_{\bf{3}}}{{\bf{H}}_{\bf{8}}}\), is a hydrocarbon that is commonly used as a fuel.
(a) Write a balanced equation for the complete combustion of propane gas.
(b) Calculate the volume of air at 25 掳C and 1.00 atmosphere that is needed to completely combust 25.0 grams of propane. Assume that air is 21.0 percent O2 by volume. (Hint: we will see how to do this calculation in a later
chapter on gases鈥攆or now use the information that 1.00 L of air at 25 掳C and 1.00 atm contains 0.275 g of O2 per liter.)
(c) The heat of combustion of propane is 鈭�2,219.2 kJ/mol. Calculate the heat of formation,螖Hf 掳of propane given that螖Hf 掳of H2O(l) = 鈭�285.8 kJ/mol and螖Hf 掳of CO2(g) = 鈭�393.5 kJ/mol.
(d) Assuming that all of the heat released in burning 25.0 grams of propane is transferred to 4.00 kilograms of water, calculate the increase in temperature of the water.
Question 11: A piece of unknown solid substance weighs 437.2 g, and requires 8460 J to increase its temperature from 19.3 掳C to 68.9 掳C.
(a) What is the specific heat of the substance?
(b) If it is one of the substances found in Table 5.1, what is its likely identity?
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.
When 0.963 g of glucose, C6H6, is burned in a bomb calorimeter, the temperature of the calorimeter increases by 8.39掳C. The bomb has a heat capacity of 784 J/掳C and is submerged in 925 mL of water. How much heat was produced by the combustion of the glucose sample?
When 50.0g of 0.200M NaCl(aq) at 24.1藲C is added to 100.0g of 0.100M AgNO3(aq) at 24.1藲C in a calorimeter, the temperature rises to 25.2藲C as AgCl(s) forms. Assuming the specific heat of the solution and products is 4.20J/g藲C, calculate the approximate amount of heat in joules produced.
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