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For a chemical reaction, the standard G...

For a chemical reaction, the standard Gibbs energy change, `DeltaG^(@)` is - `7.64xx10^(4)` J `"mol"^(-1)` . What is the value of equilibrium constant (K) ?

A

`K=1`

B

`K gt 1`

C

`K lt 1`

D

`K=0`

Text Solution

Verified by Experts

The correct Answer is:
B
Standard Gibbs free energy,
`DeltaG^(@)=-2.303` RT log K
Given, `DeltaG^(@)=-7.64xx10^(4)`J/mol
`log K=-(DeltaG^(@))/(2.303RT)`
`K=` antilog`-((DeltaG^(@))/(2.303 RT))`
`K=` antilog`-(((-)7.64xx10^(4))/(2.303xx8.314xx298))`
Here, K is greater than one.
Thus, option (b) is correct.
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