What will be the effect on the equilibrium constant for the reaction `N_(2)+3H_(2)hArr2NH_(3),`
`DeltaH=-22.4` kcal, when
a. Pressure is increased
b. Concentration of `N_(2)` is increased and
c. Temperature is raised at equilibrium ?

Explanation

To determine the effect on the equilibrium constant for the reaction \( N_2 + 3H_2 \rightleftharpoons 2NH_3 \) with \( \Delta H = -22.4 \) kcal, we will analyze the effects of changes in pressure, concentration of \( N_2 \), and temperature.

### Step-by-Step Solution:

1. **Understanding the Reaction**:
The reaction is the formation of ammonia from nitrogen and hydrogen. It is an exothermic reaction since \( \Delta H \) is negative.

2. **Effect of Pressure Increase**:
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