For a reaction, `DeltaH=10000" kJ "mol^(-1) and DeltaS=25" kJ "k^(-1)mol^(-1)`. The minimum temperature, above which the reaction would be spontaneous is

Options

A. `127^(@)C`
B. `400^(@)C`
C. `75^(@)C`
D. `410^(@)C`

Answer

A

Explanation

As per the equation, `Delta=DeltaH-TDeltaS`, for `DeltaG` to be negative `TDeltaS` should be greater than `DeltaH` i.e., `TDeltaS gt DeltaH`
or `T gt (DeltaH)/(DeltaS)=(1000)/(25)=400K` or `127^(@)C`
`therefore`The minimum temperature above which the reaction is spotaneous is `127^(@)C`