Chapter 17, Problem 56A

Interpretation Introduction

Interpretation:

The effect of increase in temperature needs to be explained on the equilibrium position of the reaction in which heat is produced.

Concept introduction:

According to Le Chatelier’s principle, when concentration of the reactants and products are changed then equilibrium position is also changes. As lowering the temperature the equilibrium is also shifts towards the right side or product side and more products are formed. So, there is a stress on equilibrium by increasing or decreasing of the concentration of reactants and products.

Answer to Problem 56A

When temperature increases and heat produces as a product then the equilibrium of the reaction shifts to the left side or reactant side.

Explanation of Solution

Given information:

${\text{PCl}}_{\text{5}}{\left(\text{g}\right)}_{}\underset{}{\rightleftharpoons }{\text{ PCl}}_{\text{3}}\left(\text{g}\right){\text{ + Cl}}_{\text{2}}{\left(\text{g}\right)}_{}\text{+ heat}$ When temperature is increased and heat is produced as a product then the equilibrium of the reaction shifts to the left side or reactant side.

According to Le Chatelier’s principle, by changing the temperature the equilibrium position is also changes.

In case of exothermic reaction, the heat is in product side. On increasing temperature, product is increased so reaction shifts in opposite direction that is backward or reactant side.

Conclusion

When temperature increases and heat produces as a product then the equilibrium of the reaction shifts to the left side or reactant side.