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For a reaction R(1), DeltaG = xkJ//mol. ...

For a reaction `R_(1), DeltaG = xkJ//mol`. For a reaction `R_(2), Delta G = y K J//mol.` Reaction `R_(1)`, is non-spontaneous but along with `R_(2)` it is spontaneous. This means that

A

x is negative, y is positive but in magnitude `x gt y`

B

x is positive, y is negative but in magnitude `y gt x`

C

both x and y are negative but not equal

D

both x and y are positive but not equal

Text Solution

Verified by Experts

The correct Answer is:
B
For `R_(2), Delta G` should be negative and greater than positive value of `Delta G` for `R_(1)` in magnitude.
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