Gibbs free energy equilibrium constant 2

Chemistry Level pending

The equilibrium constant of the following chemical reaction is 1.1 × 1 0 28 : 1.1 \times 10^{28}: 3 ClO − ( a q ) → 2 Cl − ( a g ) + ClO 3 − ( a g ) . 3 \text{ClO}^{-} (aq) \rightarrow 2\text{Cl}^{-} (ag) + \text{ClO}_{3}^{-} (ag). Then what is the Gibbs free energy of this reaction at 25.0 25.0 °C when 1.0 1.0 mol of ClO 3 − ( a g ) \text{ClO}_{3}^{-} (ag) is produced from the reaction?

160.01 kJ 160.01\text{ kJ} − 160.01 kJ -160.01\text{ kJ} 53.33 kJ 53.33\text{ kJ} − 53.33 kJ -53.33\text{ kJ}

Krishna Singh by Krishna Singh , 22, India

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