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 2Hg(l)+O2(g)→2HgO(s)2 \mathrm{Hg}(l) + \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{HgO}(s), we need to determine if entropy increases or decreases. Entropy (SS) generally increases with an increase in the number of gas molecules. Here, the reaction goes from one gas molecule (O2\mathrm{O}_{2}) to none, indicating a decrease in entropy.

Step 2: Determine Spontaneity of the Reaction

The reaction has ΔH=−43kcal/mol\Delta H = -43 \mathrm{kcal/mol}, which is exothermic. Spontaneity is determined by the Gibbs free energy change (ΔG\Delta G), which depends on both enthalpy and entropy. Without specific ΔS\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 (EactE_{\text{act}}) is generally faster. Here, the reaction with Eact=+5kcal/molE_{\text{act}} = +5 \mathrm{kcal/mol} is faster than the one with Eact=+10kcal/molE_{\text{act}} = +10 \mathrm{kcal/mol}.

Final Answer

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