Questions: For the reaction 2 Hg(l)+O2(g) -> 2 HgO(s), ΔH=-43 kcal / mol. (a) Does entropy increase or decrease in this process? (b) Is this process spontaneous? Which reaction is faster, one with Eact =+10 kcal / mol or one with Eact =+5 kcal / mol ? Explain. Why does increasing concentration generally increase the rate of a reaction? If a catalyst changes the activation energy of a forward reaction from 28.0 kcal / mol to 23.0 kcal / mol, what effect does it have on the reverse reaction? For the reaction 2 H2(g)+2 C(s) -> H2C=CH2(g), ΔG=+16.3 kcal / mol at 25°C (a) Is the reaction of hydrogen with carbon to yield ethylene spontaneous at 25 C ? (b) Is it possible to find a catalyst for the reaction of hydrogen with carbon at 25 C ? Write the equilibrium equations for the following reactions, and tell whether reactants or products are favored in each case. (a) S2(g)+2 H2(g) <=> 2 H2S(g) K=2.8 x 10^21 (b) CO(g)+2 H2(g) CH3OH(g) K=10.5 (c) AgCl(s)+H2O(l) <=> Ag+(aq)+Cl^-(aq) K=1.3 x 10^-23

For the reaction 2 Hg(l)+O2(g) -> 2 HgO(s), ΔH=-43 kcal / mol. (a) Does entropy increase or decrease in this process? (b) Is this process spontaneous? Which reaction is faster, one with Eact =+10 kcal / mol or one with Eact =+5 kcal / mol ? Explain. Why does increasing concentration generally increase the rate of a reaction? If a catalyst changes the activation energy of a forward reaction from 28.0 kcal / mol to 23.0 kcal / mol, what effect does it have on the reverse reaction? For the reaction 2 H2(g)+2 C(s) -> H2C=CH2(g), ΔG=+16.3 kcal / mol at 25°C (a) Is the reaction of hydrogen with carbon to yield ethylene spontaneous at 25 C ? (b) Is it possible to find a catalyst for the reaction of hydrogen with carbon at 25 C ? Write the equilibrium equations for the following reactions, and tell whether reactants or products are favored in each case. (a) S2(g)+2 H2(g) <=> 2 H2S(g) K=2.8 x 10^21 (b) CO(g)+2 H2(g) CH3OH(g) K=10.5 (c) AgCl(s)+H2O(l) <=> Ag+(aq)+Cl^-(aq) K=1.3 x 10^-23
Transcript text: For the reaction $2 \mathrm{Hg}(l)+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{HgO}(\mathrm{s}), \Delta \mathrm{H}=-43 \mathrm{kcal} / \mathrm{mol}$. (a) Does entropy increase or decrease in this process? (b) Is this process spontaneous? Which reaction is faster, one with Eact $=+10 \mathrm{kcal} / \mathrm{mol}$ or one with Eact $=+5 \mathrm{kcal} / \mathrm{mol}$ ? Explain. Why does increasing concentration generally increase the rate of a reaction? If a catalyst changes the activation energy of a forward reaction from $28.0 \mathrm{kcal} / \mathrm{mol}$ to $23.0 \mathrm{kcal} / \mathrm{mol}$, what effect does it have on the reverse reaction? For the reaction $2 \mathrm{H}_{2}(\mathrm{~g})+2 \mathrm{C}(\mathrm{s}) \rightarrow \mathrm{H}_{2} \mathrm{C}=\mathrm{CH}_{2}(\mathrm{~g}), \Delta \mathrm{G}=+16.3 \mathrm{kcal} / \mathrm{mol}$ at $25^{\circ} \mathrm{C}$ (a) Is the reaction of hydrogen with carbon to yield ethylene spontaneous at 25 C ? (b) Is it possible to find a catalyst for the reaction of hydrogen with carbon at 25 C ? Write the equilibrium equations for the following reactions, and tell whether reactants or products are favored in each case. (a) $\mathrm{S}_{2}(\mathrm{~g})+2 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{H} 2 \mathrm{~S}(\mathrm{~g}) \mathrm{K}=2.8 \times 10^{21}$ (b) $\mathrm{CO}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{~g}) \quad \mathrm{CH}_{3} \mathrm{OH}(\mathrm{g}) \quad \mathrm{K}=10.5$ (c) $\mathrm{AgCl}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightleftharpoons \mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq}) \mathrm{K}=1.3 \times 10^{-23}$
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Solution

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Solution Steps

Step 1: Analyze Entropy Change in the Reaction

For the reaction \(2 \mathrm{Hg}(l) + \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{HgO}(s)\), we need to determine if entropy increases or decreases. Entropy (\(S\)) generally increases with an increase in the number of gas molecules. Here, the reaction goes from one gas molecule (\(\mathrm{O}_{2}\)) to none, indicating a decrease in entropy.

Step 2: Determine Spontaneity of the Reaction

The reaction has \(\Delta H = -43 \mathrm{kcal/mol}\), which is exothermic. Spontaneity is determined by the Gibbs free energy change (\(\Delta G\)), which depends on both enthalpy and entropy. Without specific \(\Delta S\) and temperature values, we can't definitively determine spontaneity, but exothermic reactions often tend to be spontaneous at lower temperatures.

Step 3: Compare Reaction Rates Based on Activation Energy

The reaction with a lower activation energy (\(E_{\text{act}}\)) is generally faster. Here, the reaction with \(E_{\text{act}} = +5 \mathrm{kcal/mol}\) is faster than the one with \(E_{\text{act}} = +10 \mathrm{kcal/mol}\).

Final Answer

  • (a) Entropy decreases in this process: \(\boxed{\text{Entropy decreases}}\)
  • (b) The process is likely spontaneous at lower temperatures due to being exothermic: \(\boxed{\text{Possibly spontaneous}}\)
  • The reaction with \(E_{\text{act}} = +5 \mathrm{kcal/mol}\) is faster: \(\boxed{\text{Reaction with } E_{\text{act}} = +5 \mathrm{kcal/mol} \text{ is faster}}\)
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