Question

For a reversible equilibrium reaction $K_C>K_P$ at $298K$ and $\Delta H=+200$ $KJ$, the forward reaction is favoured if:
(i) Pressure is increased
(ii) Temperature is increased
(iii) Temperature is decreased
(iv) Increasing the concnetration of reactants

• A. i, ii, iv
• B. i, ii
• C. ii, iv
• D. i, iii, iv

Answer 1

The correct option is A i, ii, iv

As $K_c>K_p$.

$K_p=K_c{\left(RT\right)}^{\Delta n}$

$⟹\Delta n<1⟹$ number of reactants > number of products

So, when pressure is increased, reaction favours towards less number of moles, i.e., forward reaction.

As, the concentration of reactants is increased, it moves in the forward direction.

As the reaction is endothermic, increase in temperature favours forward reaction.