`N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g), DeltaH^(ɵ)=-22.4 kJ`
The pressure inside the chamber is `100` atm and temperature at `300 K`
On adding catalyst the equilibrium of reaction:

Options

A. Shift in backward direction
B. Shift in forward direction
C. Does not affect the equilibrium
D. Cannot predict.

Answer

To solve the question regarding the effect of a catalyst on the equilibrium of the reaction \( N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \) under the given conditions, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Reaction**: The reaction provided is the formation of ammonia from nitrogen and hydrogen gases. The reaction is exothermic, as indicated by the negative enthalpy change (\( \Delta H^{\circ} = -22.4 \, \text{kJ} \)).

2. **Identify the Role of a Catalyst**: A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the process. It does this by providing an alternative pathway for the reaction with a lower activation energy.

3. **Effect of Catalyst on Equilibrium**: While a catalyst speeds up the rate at which equilibrium is reached, it does not change the position of the equilibrium or the equilibrium constant. This means that the concentrations of reactants and products at equilibrium remain the same, regardless of the presence of a catalyst.

4. **Conclusion**: Since the catalyst does not affect the equilibrium position or the equilibrium constant, the equilibrium of the reaction will remain unchanged after the addition of the catalyst. It will only allow the system to reach equilibrium faster.

### Final Answer:
The addition of a catalyst does not affect the equilibrium position of the reaction \( N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \). It only helps the system to reach equilibrium more quickly.