Hydrolysis of sucrose is given by the following reaction.
`Sucrose+ H_2O rarr Glucose` + Fructose If the equilibrium constant `(K_c)` is `2xx10^13` at `300 K` the value of `delta_r G^theta` at the same temperature will be:

Options

A. `-8.314 "Jmol"^(-1)K^(-1) xx 300K xx In(2xx10^(13))`
B. `8.314 "Jmol"^(-1)K^(-1) xx 300K xx In(2xx10^(13))`
C. `8.314 "Jmol"^(-1)K^(-1) xx 300K xx In(3xx10^(13))`
D. `-8.314 "Jmol"^(-1)K^(-1) xx 300K xx In(4xx10^(13))`

Answer

A

Explanation

`DeltaG = DeltaG^@ +RT ` ln Q
At equilibrium `DeltaG = 0 , Q = K_(eq)`
So `Delta_rG^@=-RTlnK_(eq)`
`Delta_rG^@=8.314 "Jmol"^(-1)K^(-1) xx 300K xx ln(2xx10^(13))`