Q.For the equilibrium $2NO_2(g) \rightleftharpoons N_2O_4(g)$ , $\Delta H = -58 \text{ kJ}$ . This equilibrium can be shifted to the left by:

Decreasing temperature

Increasing pressure

Increasing temperature

Adding an inert gas at constant volume

The correct solution involves applying the fundamental concept to derive the final value step by step...

Already a member? Login here

Q.For the equilibrium 2NO2(g)⇌N2O4(g)2NO_2(g) \rightleftharpoons N_2O_4(g)2NO2​(g)⇌N2​O4​(g), ΔH=−58 kJ\Delta H = -58 \text{ kJ}ΔH=−58 kJ. This equilibrium can be shifted to the left by: