Question

$N_2{F}_4\left(g\right)\rightleftharpoons 2N{F}_2\left(g\right);\Delta H^o=38.5kJ$. Which of the following conditions will favour the formation of $N{F}_2$?

• A. Adding He to the equilibrium mixture at constant temperature and volume.
• B. Increasing the temperature.
• C. $N{F}_2$ gas is removed from the reaction mixture.
• D. Decreasing the pressure at constant temperature.

Answer 1

Answer: (B), (C), (D)

The correct options are
B Increasing the temperature.
C $N{F}_2$ gas is removed from the reaction mixture.
D Decreasing the pressure at constant temperature.

When helium is added at constant volume and temperature, there is no effect on the equilibrium of the reaction.
The forward reaction is an endothermic reaction. It will be favoured by an increase in temperature.
When $N{F}_2$ gas is removed from the reaction mixture, more and more $N{F}_2$ gas will be formed as the reaction will shift in the forward direction.
The forward reaction occurs with decrease in the number of moles. When pressure is decreased, the equilibrium will shift in the forward direction so that the number of moles increases which will increase the pressure.