Question

The equilibrium constant $K_c$ or $K_p$ for endothermic reaction increases with

• A. Increase in temperature
• B. Decreases in temperature
• C. No effect of temperature
• D. Increases in pressure

Answer 1

The correct option is A Increase in temperature

Increase in temperature favours the endothermic reaction and decrease in temperature favours the exothermic reaction for the forward reaction.
Means for exothermic reactions, the value of $K_c$ and $K_p$ decrease with rise in temperature while for endothermic reactions, the value of $K_c$ and $K_p$ increases with rise in temperature. This type of variation in equilibrium constant with temperature was given by Van't Hoff equation as follows
$log{K}_2-log{K}_1=\frac{△H}{2.303R}[\frac{1}{T_1}-\frac{1}{T_2}]$
or log $\frac{K_2}{K_1}=\frac{△H}{2.303R}[\frac{1}{T_1}-\frac{1}{T_2}]$
Where,
$K_2=$ equlibrium constant at temperature $T_2$
$K_1=$ equilibrium constant at temperature $T_1$