Chapter 5: Problem 19
(a) What is work? (b) How do we determine the amount of work done, given the force associated with the work?
Chapter 5: Problem 19
(a) What is work? (b) How do we determine the amount of work done, given the force associated with the work?
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Get started for freeThe heat of combustion of fructose, \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\), is \(-2812 \mathrm{~kJ} / \mathrm{mol}\). If a fresh golden delicious apple weighing \(4.23\) oz \((120 \mathrm{~g})\) contains \(16.0 \mathrm{~g}\) of fructose, what caloric content does the fructose contribute to the apple?
Which will release more heat as it cools from \(50^{\circ} \mathrm{C}\) to \(25^{\circ} \mathrm{C}, 1 \mathrm{~kg}\) of water or \(1 \mathrm{~kg}\) of aluminum? How do you know? [Section 5.5]
From the enthalpies of reaction \(2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(g) \quad \Delta H=-483.6 \mathrm{~kJ}\) \(3 \mathrm{O}_{2}(g) \stackrel{-\cdots}{\longrightarrow} 2 \mathrm{O}_{3}(g) \quad \Delta H=+284.6 \mathrm{~kJ}\) calculate the heat of the reaction $$ 3 \mathrm{H}_{2}(g)+\mathrm{O}_{3}(g) \longrightarrow 3 \mathrm{H}_{2} \mathrm{O}(g) $$
Consider the following unbalanced oxidation-reduction reactions in aqueous solution: $$ \begin{aligned} \mathrm{Ag}^{+}(a q)+\mathrm{Li}(s) & \longrightarrow \mathrm{Ag}(s)+\mathrm{Li}^{+}(a q) \\ \mathrm{Fe}(s)+\mathrm{Na}^{+}(a q) & \longrightarrow \mathrm{Fe}^{2+}(a q)+\mathrm{Na}(s) \\ \mathrm{K}(s)+\mathrm{H}_{2} \mathrm{O}(l) & \longrightarrow \mathrm{KOH}(a q)+\mathrm{H}_{2}(g) \end{aligned} $$ (a) Balance each of the reactions. (b) By using data in Appendix \(C\), calculate \(\Delta H^{\circ}\) for each of the reactions. (c) Based on the values you obtain for \(\Delta H^{\circ}\), which of the reactions would you expect to be thermodynamically favored? (That is, which would you expect to be spontaneous?) (d) Use the activity series to predict which of these reactions should occur. ono (Section 4.4) Are these results in accord with your conclusion in part (c) of this problem?
Burning methane in oxygen can produce three different carbon-containing products: soot (very fine particles of graphite), \(\mathrm{CO}(\mathrm{g})\), and \(\mathrm{CO}_{2}(\mathrm{~g})\). (a) Write three balanced equations for the reaction of methane gas with oxygen to produce these three products. In each case assume that \(\mathrm{H}_{2} \mathrm{O}(l)\) is the only other product. (b) Determine the standard enthalpies for the reactions in part (a). (c) Why, when the oxygen supply is adequate, is \(\mathrm{CO}_{2}(g)\) the predominant carbon- containing product of the combustion of methane?
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