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  • Hydrolysis of sucrose is given by the following reaction: <img alt="Sucrose +H_{2}O \rightleftharpoons Glucose + Fructose" src="https://entrancecorner.oncodecogs.com/gif.latex?Sucrose%20&

Hydrolysis of sucrose is given by the following reaction:

Sucrose +H_{2}O \rightleftharpoons Glucose + Fructose

If the equilibrium constant  (K_{c}) is 2\times 10^{13} at 300K, the value of \Delta _{r}G^{\Theta } at the same temprature will be:

 

Option: 1

-8.314Jmol^{-1}K^{-1}\times 300K \times ln (4\times 10^{13})


Option: 2

-8.314Jmol^{-1}K^{-1}\times 300K \times ln (2\times 10^{13})


Option: 3

8.314Jmol^{-1}K^{-1}\times 300K \times ln (2\times 10^{13})


Option: 4

8.314Jmol^{-1}K^{-1}\times 300K \times ln (3\times 10^{13})


Answers (1)

best_answer

The chemical reaction occurs as follows:

\text { Sucrose }+\mathrm{H_{2} O} \: \rightleftharpoons \: \text {Glucose + fructose }

\mathrm{k_{c}=2 \times 10^{13} \text { at } 300 \mathrm{K}}

Now, \mathrm{\Delta _{r}G^{o}} is given as :

\mathrm{\Delta_{r} G^{0}=-\: R T \ln K_{c}}

\Delta_{r} G^{0}=-\: 8.31 \times 300 \ln \left(2 \times 10^{13}\right)

Therefor, Option (2) is correct.

 

Posted by

jitender.kumar

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