1. How is the value of Kp affected when the temperature is increased given that change in enthalpy of the reaction is positive? Explain (2) 2. Mention three actors that affect the spontaneity of the reaction. (3) 3. For which of these processes would ?S be expected to be most positive? (2) A Fe(s) ? Fe(l) B Fe(s) + S(s) ? FeS(s) C 2Fe(s) + 3/2 O2(g) ? Fe2O3 (s) D HF(l) ? HF(g) E 2H2O2(l) ? 2H2O(l) + O2(g)
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An increase in temperature shifts the equilibrium position in the direction that absorbs heat. For an endothermic reaction (\( \Delta H > 0 \)), the equilibrium shifts to the right, increasing the value of \( K_{p} \). Show more…
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For the reaction $$ \mathrm{C}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{CO}_{2}(\mathrm{~g}) $$ $\Delta H^{0}=-393.51 \mathrm{~kJ} / \mathrm{mol}$ and $\Delta S^{0}=2.86 \mathrm{~J} / \mathrm{mol} \cdot \mathrm{K}$ at $25^{\circ} \mathrm{C} .$ (a) Does this reaction become more or less favorable as the temperature increases? (b) For the reaction $$ \mathrm{C} 1 \mathrm{~s} 2+\frac{1}{2} \mathrm{O}_{2} 1 \mathrm{~g} 2 \longrightarrow \mathrm{CO} 1 g 2 $$ $\Delta H^{0}=-110.52 \mathrm{~kJ} / \mathrm{mol}$ and $\Delta S^{0}=89.36 \mathrm{~J} / \mathrm{mol} \cdot \mathrm{K}$ at $25^{\circ} \mathrm{C} .$ Does this reaction become more or less favorable as the temperature increases? (c) Compare the temperature dependencies of these reactions.
For Exercises 17.87 to 17.102 , assume that $\Delta H^{\circ}$ and $\Delta S^{\circ}$ do not change with temperature. State whether increasing temperature increases or decreases the value of the equilibrium constant for the following reactions. (a) $\mathrm{N}_{2} \mathrm{O}(\mathrm{g})+\mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{N}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\ell)$ (b) $\mathrm{CO}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{COCl}_{2}(\mathrm{~g})$ (c) $\mathrm{CO}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{HCOOH}(\mathrm{g})$ (d) $\mathrm{PCl}_{5}(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g})$ (e) $2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_{3}(\mathrm{~g})$
For the reaction $$ \begin{array}{c} \mathrm{C}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{CO}_{2}(\mathrm{~g}) \\ \Delta H^{0}=-393.51 \mathrm{~kJ} / \mathrm{mol} \text { and } \Delta S^{0}=2.86 \mathrm{~J} / \mathrm{mol} \cdot \mathrm{K} \text { at } \end{array} $$ $25^{\circ} \mathrm{C}$. (a) Does this reaction become more or less favorable as the temperature increases? (b) For the reaction $$ \begin{array}{c} \mathrm{C}(\mathrm{s})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{CO}(\mathrm{g}) \\ \Delta H^{0}=-110.52 \mathrm{~kJ} / \mathrm{mol} \text { and } \Delta S^{0}=89.36 \mathrm{~J} / \mathrm{mol} \cdot \mathrm{K} \text { at } \end{array} $$ $25^{\circ} \mathrm{C}$. Does this reaction become more or less favorable as the temperature increases? (c) Compare the temperature dependencies of these reactions.
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