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Chapter 54: Problem 5

How does temperature affect the equilibrium \(\mathrm{H}_{2} \mathrm{O}(\boldsymbol{l}) \rightleftharpoons \mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) ? Explain in terms of \(\Delta H^{\circ}\).

Short Answer

Expert verified
For the endothermic reaction \(\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{2} \mathrm{O}(g)\), an increase in temperature will shift the equilibrium towards the gaseous water, while a decrease in temperature will shift it towards the liquid water. This is in line with Le Chatelier's Principle, as the system adjusts to counter the temperature change by favoring the reaction that absorbs or releases heat.

Step by step solution

01

Identify the Type of Reaction

Identify the type of reaction based on the enthalpy change. In this case, the reaction \(\mathrm{H}_2 \mathrm{O}(l) \rightleftharpoons \mathrm{H}_2 \mathrm{O}(g)\) is endothermic because liquid water absorbs heat to become gaseous water vapor.
02

Understand the Effect of Temperature on Equilibrium

Based on Le Chatelier's Principle, for an endothermic reaction, an increase in temperature will shift the equilibrium towards the product side, and a decrease in temperature will shift the equilibrium towards the reactants side.
03

Explain the Influence of Temperature on the Given Reaction

So, for the reaction \(\mathrm{H}_2 \mathrm{O}(l) \rightleftharpoons \mathrm{H}_2 \mathrm{O}(g)\), if the temperature is increased, the reaction will shift to the right (towards gaseous water), meaning more liquid water will be converted to water vapor to absorb the added heat. If the temperature is decreased, the reaction will shift to the left (towards liquid water), signaling condensation of water vapor back to liquid form to release heat and counteract the decrease in temperature.

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Most popular questions from this chapter

Recall that \(\Delta G^{\circ}\) can be written as a function of \(\Delta H^{\circ}\) and \(\Delta S^{\circ} .\) Assume that \(\Delta H^{\circ}\) and \(\Delta S^{\circ}\) are not temperature dependent and answer each of the following: a) Derive an expression relating \(\ln K, \Delta H^{\circ}\), and \(\Delta S^{\circ} .\) That is, derive an expression that looks like \(\ln K=\) some function of \(\Delta H^{\circ}\) and \(\Delta S^{\circ}\). The temperature, \(T\), should appear only once in this equation. b) How are the equilibrium constants for reactions with \(\Delta H^{\circ}>0\) affected by an increase in temperature? c) How are equilibrium constants for reactions with \(\Delta H^{\circ}<0\) affected by an increase in temperature?
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