Equilibrium constant, `K_(c) " for the reaction" , N_(2) (g) + 3 H_(2) (g) hArr 2 NH_(3) (g) " at " 500 K " is " 0*061.` At a particular time, the analysis shows that composition of the reaction mixture is `3*0" mol "L^(-1) N_(2), 2*0 " mol "L^(-1) H_(2) and 5*0 "mol " L^(-1) NH_(3). ` Is the reaction at equilibrium ? If not , in which direction does the reaction tend to reach equilibrium ?

Explanation

To determine whether the reaction is at equilibrium and in which direction it tends to move, we can follow these steps:

### Step 1: Write the balanced chemical equation
The balanced chemical equation for the reaction is:
\[ \text{N}_2(g) + 3 \text{H}_2(g) \rightleftharpoons 2 \text{NH}_3(g) \]

### Step 2: Write the expression for the equilibrium constant \( K_c \)
The equilibrium constant \( K_c \) for the reaction is given by the formula:
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