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A+BtoC+D DeltaH=-10,000 J mol^(-1) D...

`A+BtoC+D`
`DeltaH=-10,000 J mol^(-1)`
`DeltaS-33.3 J mol^(-1)K^(-1)`
At what temperature the reaction will occur spontaneous from left to right ?

A

`=300.3K`

B

`gt300.3K`

C

`lt300.3K`

D

None of these

Text Solution

Verified by Experts

The correct Answer is:
C
`DeltaG=0=0Delta-TDeltaS`
`T=(-10000)/(-3.3)=300.3K` Since `DeltaH&DeltaH` both are negative therefore reaction will be sportaneous at `Tlt300.3K`
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