Hydrolysis of sucrose is given by the following reaction.Sucrose + H2O ⇌ Glucose + FructoseIf the equilibrium constant (Kc) is 2 $ \times $ 1013 at 800 K, the value of $\Delta r{G^\Theta }$ at the same temperature will be :

Question

Hydrolysis of sucrose is given by the following reaction.
Sucrose + H₂O ⇌ Glucose + Fructose
If the equilibrium constant (K_c) is 2 $ \times $ 10¹³ at 800 K, the value of $\Delta r{G^\Theta }$ at the same temperature will be :

8.314 J $mo{l^{ - 1}}{K^{ - 1}} \times 300K \times In(2 \times {10^{13}})$

8.314 J $mo{l^{ - 1}}{K^{ - 1}} \times 300K \times In(3 \times {10^{13}})$

$ - $ 8.314 J $mo{l^{ - 1}}{K^{ - 1}} \times 300K \times In(4 \times {10^{13}})$

-8.314 J $mo{l^{ - 1}}{K^{ - 1}} \times 300K \times In(2 \times {10^{13}})$

Solution

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