Question

For the reaction :
$C{H}_4\left(g\right)+H_{2}O\left(g\right)\rightleftharpoons CO\left(g\right)+3H_2\left(g\right),\Delta H=+ve$
Which statement is not correct?

• A. The compression of equilibrium mixture shifts the reaction toward products
• B. A rise in temperature of equilibrium mixture shifts the reaction towards products
• C. Addition of an inert gas constant pressure shifts the reaction towards products
• D. Addition of an inert gas at constant volume shifts the reaction towards reactants

Answer 1

Answer: (A), (D)

The correct options are
A The compression of equilibrium mixture shifts the reaction toward products
D Addition of an inert gas at constant volume shifts the reaction towards reactants

If we increase the pressure of this given system the equilibrium shifts in backward direction as there are less number of moles in the reactants.
The addition of inert gas at constant volume will have no effect at the equilibrium.

So here Option A and D are incorrect statements.