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

Question

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

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

Monjur Alahi

4 views

2025-01-04 04:42

1 Answers

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Salim Ahmed Kawsar · Accepted Answer · 2023-02-05T15:29:48+06:00

Salim Ahmed Kawsar

Correct Answer - A
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`

4 views Answered 2023-02-05 15:29