`DeltaG^@ "for" 1/2 N_2(g) +3/2H_2(g)hArrNH_3(g) " ""is"" " -16.5 KJ" "mol^(1)` . Find out `K_p` for the reaction at `25^@C` . Also report `K_p and DeltaG^@ "for" N_2(g) +3H_2(g) hArr 2NH_3(g) "at" 25^@C`.
Text Solution
AI Generated Solution
To solve the problem, we need to find the equilibrium constant \( K_p \) for the reaction \( \frac{1}{2} N_2(g) + \frac{3}{2} H_2(g) \rightleftharpoons NH_3(g) \) at \( 25^\circ C \) given that \( \Delta G^0 = -16.5 \, \text{kJ/mol} \). We will also find \( K_p \) and \( \Delta G^0 \) for the reaction \( N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \).
### Step 1: Convert \( \Delta G^0 \) to Joules
Given:
\[
\Delta G^0 = -16.5 \, \text{kJ/mol}
\]
Convert this to Joules:
...
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