For the reaction at 300 K , `A(g) rarr B(g) + E(g), DeltaH^(@) = -30 KJ mol^(-1)` , the decrease in standard entropy is `0.1 KJK^(-1)mol^(-1)`.The equilibrium constant K for the reaction is ________.

Explanation

To find the equilibrium constant \( K \) for the reaction \( A(g) \rightleftharpoons B(g) + E(g) \) at 300 K, we will use the given values for the change in enthalpy (\( \Delta H^\circ \)) and the change in entropy (\( \Delta S^\circ \)).

### Step-by-step Solution:

1. **Identify the given values:**
- \( \Delta H^\circ = -30 \, \text{kJ/mol} \)
- \( \Delta S^\circ = -0.1 \, \text{kJ/(K·mol)} \)
- Temperature \( T = 300 \, \text{K} \)
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