Questions: The water-gas shift reaction CO(g)+H2O(g) ⇌ CO2(g)+H2(g) is used industrially to produce hydrogen. The reaction enthalpy is ΔH∘=−41 kJ. Part A To increase the equilibrium yield of hydrogen would you use high or low temperature? We would use temperature. For an reaction such as this, temperature increases the value of K and the amount of products at equilibrium.

The water-gas shift reaction CO(g)+H2O(g) ⇌ CO2(g)+H2(g) is used industrially to produce hydrogen. The reaction enthalpy is ΔH∘=−41 kJ.

Part A

To increase the equilibrium yield of hydrogen would you use high or low temperature?

We would use temperature. For an reaction such as this, temperature increases the value of K and the amount of products at equilibrium.

Transcript text: The water-gas shift reaction $\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g)$ is used industrially to produce hydrogen. The reaction enthalpy is $\Delta H^{\circ}=-41 \mathrm{~kJ}$. Part A To increase the equilibrium yield of hydrogen would you use high or low temperature? Drag the terms on the left to the appropriate blanks on the right to complete the sentences. Reset Help decreasing increasing high Iow $\square$ We would use $\square$ temperature. For an $\square$ reaction such as this, $\square$ $\square$ temperature increases the value of $K$ and the amount of products at equilibrium. endothermic exothermic

Solution

Solution Steps

Step 1: Understanding the Reaction and Enthalpy

The water-gas shift reaction is given by:

\[ \mathrm{CO}(g) + \mathrm{H}_2\mathrm{O}(g) \rightleftharpoons \mathrm{CO}_2(g) + \mathrm{H}_2(g) \]

The reaction enthalpy is $\Delta H^{\circ} = -41 \, \text{kJ}$, indicating that the reaction is exothermic. In an exothermic reaction, heat is released as the reaction proceeds.

Step 2: Applying Le Chatelier's Principle

According to Le Chatelier's Principle, if a system at equilibrium is subjected to a change in temperature, the system will adjust to counteract that change. For an exothermic reaction, increasing the temperature will shift the equilibrium to the left (towards the reactants), while decreasing the temperature will shift the equilibrium to the right (towards the products).

Step 3: Determining the Effect of Temperature on Equilibrium

To increase the equilibrium yield of hydrogen ($\mathrm{H}_2$), we want the equilibrium to shift to the right. Since the reaction is exothermic, decreasing the temperature will favor the formation of products, thus increasing the yield of hydrogen.

Final Answer

We would use $\boxed{\text{low}}$ temperature. For an $\boxed{\text{exothermic}}$ reaction such as this, $\boxed{\text{decreasing}}$ temperature increases the value of $K$ and the amount of products at equilibrium.

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