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For the reaction at 298 K : CO(g) + (1...

For the reaction at 298 K :
`CO(g) + (1)/(2) O_(2)(g) rarr CO_(2)(g), Delta H^(@) = -282.8 kJ`
Standard entropies (in `JK^(-1) mol^(-1)`) : `CO_(2)(g) = 213.6 CO(g) = 197.6 and O_(2)(g) = 205.0 Delta_(r) G^(@)` for the reaction `(kJ mol^(-1))`

A

`-306.02`

B

`-257.81`

C

306.02

D

`-157.03`

Text Solution

Verified by Experts

The correct Answer is:
B
`Delta S^(@) = S^(@) (CO_(2)) - [S^(@)(CO) + (1)/(2) S^(@)(O_(2))]`
`= 213.6 - [197.6 + (1)/(2)(205.0)]`
`= - 86.5 JK^(-1) mol^(-1)`
`Delta G^(@) = -282.8 xx 10^(3) - 298(-86.5)`
`= -257.023 kJ mol^(-1)`
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