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If the E("cell")^(@) for a given reactio...

If the `E_("cell")^(@)` for a given reaction has a negative value, then which of the following gives the correct relationships for the values of `DeltaG^(0)` and `K_(eq)`-

A

`DeltaG^(@) gt 0, K_(eq) lt1`

B

`DeltaG^(@) gt 0 , K_(eq) gt1`

C

`DeltaG^(@) lt 0, K_(eq) gt 1`

D

`DeltaG^(@) lt 0 , K_(eq) lt1`

Text Solution

Verified by Experts

The correct Answer is:
A
`DeltaG gt 0 , K_(eq) lt1`
Since, `E_("cell")^(@) gt 0, K_(eq) lt1`
Since, `E_("cell")^(@)=-ve, DeltaG^(@)=+ve" as, "DeltaG^(@)=-nFE_("cell")^(@)`
Again, `DeltaG^(@)=-Rt ln K_(eq)`
If, `DeltaG^(@)=+ve, RT ln K_(eq)=-ve`
`therefore" "lnK_(eq)=-ve.i.e,. K_(eq) lt1`
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Knowledge Check

  • If the E_(cell)^(@) for a given reaction has a negative value, then which of the following give the correct relationships for the value of DeltaG^(@) and K_(eq) -

    A
    `DeltaG^(@) gt 0, K_(eq) lt1`
    B
    `DeltaG^(@) gt 0 , K_(eq) gt 1`
    C
    `DeltaG^(@) lt 0, K_(eq) gt1`
    D
    `DeltaG^(@) lt 0, K_(eq) lt 1`

  • If the E_("cell")^(@) for a given reaction has a negative value, which of the following gives the correct relationships for the value of DeltaG^(@) and K_(eq) -

    A
    `DeltaG^(@) gt 0, K_(eq) lt1`
    B
    `DeltaG^(@) gt 0 , K_(eq) gt 1`
    C
    `DeltaG^(@) lt 0, K_(eq) gt1`
    D
    `DeltaG^(@) lt 0, K_(eq) lt 1`

  • If the E_(cell)^(0) for a given reaction has a negative value, which of the following gives the correct relationships for the values of DeltaG^(0) and K_(eq) ?

    A
    `DeltaG^(0) lt K_(eq) lt 1`
    B
    `DeltaG^(0) gt 0, K_(eq) lt 1`
    C
    `DeltaG^(0) gt 0, K_(eq) gt 1`
    D
    `DeltaG^(0) lt 0 , K_(eq) gt 1`

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