One mole of nitrogen is mixed with three moles of hydrogen in a 4 litre container. If 0.25 per cent of nitrogen is converted into ammonia by the following reaction
` N_2(g) +3H_2 hArr 2NH_3(g)`
calculate the equilibrium constant of the reaction in concentration units. What will be the value of K for the following reaction?
` (1)/(2) N_2 (g) + (3)/(2) H_2 hArr NH_3 (g)`

Explanation

To solve the problem step by step, we will first calculate the equilibrium constant \( K_c \) for the reaction:

\[ N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \]

### Step 1: Determine Initial Moles
We start with:
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