Question

The water-gas shift reaction CO(g)+H2O(g)⇌CO2(g)+H2(g) is used industrially to produce hydrogen. The reaction enthalpy is ΔH∘=−41kJ.Part ATo 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 sentenceshighexothermiclowendothermicdecreasingincreasingWe would use We would use blanktemperature. For an blankreaction such as this, blanktemperature increases the value of Kand the amount of products at equilibrium. temperature. For an We would use blanktemperature. For an blankreaction such as this, blanktemperature increases the value of Kand the amount of products at equilibrium. reaction such as this, We would use blanktemperature. For an blankreaction such as this, blanktemperature increases the value of Kand the amount of products at equilibrium. temperature increases the value of K and the amount of products at equilibrium.

Answer 1

Answer:

To increase the yield of H₂ we would use a low temperature.

For an exothermic reaction such as this, decreasing temperature increases the value of K and the amount of products at equilibrium. Low temperature increases the value of K and the amount of products at equilibrium.

Explanation:

Let´s consider the following reaction:

CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g)

When a system at equilibrium is disturbed, the response of the system is explained by Le Chatelier's Principle: If a system at equilibrium suffers a perturbation (in temperature, pressure, concentration), the system will shift its equilibrium position to counteract such perturbation.

In this case, we have an exothermic reaction (ΔH° < 0). We can imagine heat as one of the products. If we decrease the temperature, the system will try to raise it favoring the forward reaction to release heat and, at the same time, increasing the yield of H₂. By having more products, the value of the equilibrium constant K increases.