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For the reaction CO(g)+1/2O(2)(g) rarr C...

For the reaction `CO_(g)+1/2O_(2)(g) rarr CO_(2)(g), DeltaH and DeltaS` are -283 k J and -87 `JK^(-1)`, respectively. It was intended to carry out this reaction at 1000, 1500, 3000 and 3500 K. At which of these temperatures would this reaction be thermodynamically spontaneous ?

A

1500 and 3500 K

B

3000 and 3500 K

C

1000, 1500 and 3000 K

D

At all these temperatures

Text Solution

Verified by Experts

The correct Answer is:
C
`because DeltaG=DeltaH-T*DeltaS`
For a spontaneous reaction `DeltaG` should be negative
`" "DeltaH=-238kJ, DeltaS=-87JK^(-1)`
Hence, reaction will be spontaneous when `DeltaH gt T*DeltaS`. Therefore, at 1000, 1500 and 3000 K the reaction would be spontaneous.
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