For the reaction
`CO (g) + (1)/(2) O_(2) (g) rarr CO_(2) (g)`
`Delta H` and `Delta S` are `-283 kJ` and `-87 J K^(-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?

Options

A. 1500 and 3500K
B. 3000 and 3500 K
C. 1000, 1500 and 3000 K
D. 1500, 3000 and 3500 K

Answer

C

Explanation

`:.DeltaG-DeltaH-TDeltaS`
For a spontaneous reaction `DeltaG` should be negative
`DeltaH=-234kJ,DeltaS=-87JK^(-1)`
Hence reaction will be spontaneous when `DeltaHgtT.DeltaS`.
Therefore at 1000, 1500 and 3000 K the reaction would be spontaneous.