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Question

A change in the free energy of a system at constant temperature and pressure will be:
ΔsysG=ΔsysHTΔsysS
At constant temperature and pressure,
ΔsysG<0 (spontaneous)
ΔsysG=0 (equilibrium)
ΔsysG>0 (nonspontaneous)
A reaction has positive values of ΔH and ΔS.
From this you can deduce that the reaction:

A
must be spontaneous at any temperature
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B
cannot be spontaneous at any temperature
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C
will be spontaneous only at low temperature
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D
will be spontaneous only at high temperature
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Solution

The correct option is D will be spontaneous only at high temperature
As we know,
ΔG=ΔHTΔS and for a spontaneous reaction,

ΔG=ve

This happens only at higher temperatures.

Therefore, D option is right.

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