A spontaneous reaction is impossible if
(a) both Δ H and Δ S are negative
(b) both Δ H and Δ S are positive
(c) Δ H is negative and Δ S is positive
(d) Δ H is positive and Δ S is negative
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A spontaneous reaction is impossible if H is positive and Δ S is negative
option (d) right
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A spontaneous reaction is impossible if (d) ΔH is positive and ΔS is negative.
Explanation:
A reaction is non-spontaneous when ΔH is positive and ΔS is negative.
When ΔH = + ve and ΔS is - ve
Now, the Gibbs free energy is given by the formula:
ΔG = ΔH - TΔS
ΔG = + ve - (T × - ve)
ΔG = positive + positive
∴ ΔG = positive
The value of the ΔG is positive during non-spontaneous process.
For spontaneous process, the Gibbs free energy is need to be negative and value of ΔH and ΔS are positive.
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