Question

Consider a reaction:
$2A\left(g\right)+3B\left(g\right)\rightleftharpoons 3C\left(g\right)+2D\left(g\right)$
When the pressure is increased :

• A. No change in equilibrium.
• B. Equilibrium is shifted in backward direction
• C. Equilibrium is shifted in forward direction
• D. None of the above

Answer 1

The correct option is A No change in equilibrium.

The equilibrium reaction is
$2A\left(g\right)+3B\left(g\right)\rightleftharpoons 3C\left(g\right)+2D\left(g\right)$.

The total number of moles of reactants is equal to the total number of moles of products .i.e. $\Delta n_g=n_{g_{products}}-n_{g_{reactants}}=(3+2)-(2+3)=0$
As the number of moles are equal, both in reactants and products side, therefore pressure has no effect on the equilibrium.
So the equilibrium will remain unchanged.