Chapter 5: Problem 11
In what two ways can an object possess energy? How do these two ways differ from one another?
Chapter 5: Problem 11
In what two ways can an object possess energy? How do these two ways differ from one another?
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Get started for freeUsing values from Appendix \(C\), calculate the standard enthalpy change for each of the following reactions: (a) \(2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(g)\) (b) \(\mathrm{Mg}(\mathrm{OH})_{2}(s) \longrightarrow \mathrm{MgO}(s)+\mathrm{H}_{2} \mathrm{O}(l)\) (c) \(\mathrm{N}_{2} \mathrm{O}_{4}(g)+4 \mathrm{H}_{2}(g) \longrightarrow \mathrm{N}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)\) (d) \(\mathrm{SiCl}_{4}(l)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{SiO}_{2}(s)+4 \mathrm{HCl}(g)\)
(a) When a 3.88-g sample of solid ammonium nitrate dissolves in \(60.0 \mathrm{~g}\) of water in a coffee-cup calorimeter (Figure 5.17), the temperature drops from \(23.0^{\circ} \mathrm{C}\) to \(18.4^{\circ} \mathrm{C}\). Calculate \(\Delta H\left(\right.\) in \(\mathrm{kJ} / \mathrm{mol} \mathrm{NH}_{4} \mathrm{NO}_{3}\) ) for the solu- tion process $$ \mathrm{NH}_{4} \mathrm{NO}_{3}(s) \rightarrow \mathrm{NH}_{4}{ }^{+}(a q)+\mathrm{NO}_{3}^{-}(a q) $$ Assume that the specific heat of the solution is the same as that of pure water. (b) Is this process endothermic or exothermic?
Naphthalene \(\left(\mathrm{C}_{10} \mathrm{H}_{8}\right)\) is a solid aromatic compound often sold as mothballs. The complete combustion of this substance to yield \(\mathrm{CO}_{2}(g)\) and \(\mathrm{H}_{2} \mathrm{O}(l)\) at \(25^{\circ} \mathrm{C}\) yields \(5154 \mathrm{~kJ} / \mathrm{mol}\). (a) Write balanced equations for the formation of naphthalene from the elements and for its combustion. (b) Calculate the standard enthalpy of formation of naphthalene.
How many grams of methane \(\left[\mathrm{CH}_{4}(g)\right]\) must be combusted to heat \(1.00 \mathrm{~kg}\) of water from \(25.0^{\circ} \mathrm{C}\) to \(90.0^{\circ} \mathrm{C}\), assuming \(\mathrm{H}_{2} \mathrm{O}(l)\) as a product and \(100 \%\) efficiency in heat transfer?
Consider the decomposition of liquid benzene, \(\mathrm{C}_{6} \mathrm{H}_{6}(l)\), to gaseous acetylene, \(\mathrm{C}_{2} \mathrm{H}_{2}(g)\) : $$ \mathrm{C}_{6} \mathrm{H}_{6}(l) \longrightarrow 3 \mathrm{C}_{2} \mathrm{H}_{2}(g) \quad \Delta H=+630 \mathrm{~kJ} $$ (a) What is the enthalpy change for the reverse reaction? (b) What is \(\Delta H\) for the formation of 1 mol of acetylene? (c) Which is more likely to be thermodynamically favored, the forward reaction or the reverse reaction? (d) If \(C_{6} \mathrm{H}_{6}(g)\) were consumed instead of \(\mathrm{C}_{6} \mathrm{H}_{6}(l)\), would you expect the magnitude of \(\Delta H\) to increase, decrease, or stay the same? Explain.
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