Question

For which of the following reactions at equilibrium at constant temperature doubling the volume will cause a shift to the right ( favour forward reaction)?

• A. $N_2{O}_4\left(g\right)\rightleftharpoons 2N{O}_2\left(g\right)$
  
• B. $2CO\left(g\right)+O_2\rightleftharpoons 2C{O}_2\left(g\right)$
  
• C. $N_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2NO\left(g\right)$
• D. All of these

Answer 1

The correct option is A $N_2{O}_4\left(g\right)\rightleftharpoons 2N{O}_2\left(g\right)$


As per Le- chatelier principle,
Doubling the volume would reduce the pressure and shift the equilibrium in the direction where there is more number of moles of gases.
So, in option (a), the equilibrium will shift to the right.
In option (b), the reaction will favour formation of reactants.
In option (c), number of moles of reactants is equal to number of moles of products.