Chapter 17, Problem 34A

Interpretation Introduction

Interpretation:The shift in the equilibrium position has to be predicted for an endothermic reaction with an increase in temperature.

Concept introduction: Reactions in which heat is absorbed are called as endothermic reaction. Endothermic reaction yield products of higher energy than the reactants.

Decomposition of calcium carbonate to give calcium oxide and carbon oxide is an example of endothermic reaction.

  $CaC{O}_3\left(s\right)+556kJ\rightleftharpoons CaO\left(s\right)+C{O}_2\left(g\right)$

Answer to Problem 34A

The shift in the equilibrium position would be towards the products.

Explanation of Solution

The given reaction is,

  $4NO\left(g\right)+6H_{2}O\left(g\right)\rightleftharpoons 4N{H}_3\left(g\right)+5O_2\left(g\right)$

The production of ammonia gas with evolution of oxygen gas from nitrogen monoxide and water is an endothermic reaction. Heat is considered as a reactant in endothermic reaction and in endothermic reactions, heat is absorbed.

In endothermic reaction, the equilibrium constant increases with an increase in temperature, therefore the reaction shifts to the right (towardsthe product).

By Le Chatelier’s principle, the increase in temperature would shift the equilibrium to the right, producing more ammonia and oxygen.

Therefore, the shift in the equilibrium position would be towards the products when there is an increase in temperature for an endothermic reaction.

Conclusion

The shift in the equilibrium position would be towards the products when there is an increase in temperature for an endothermic reaction.