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Thermodynamic Processes

A reaction ha...

Question

A reaction has positive values of $Δ H$ and $Δ S$ . 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,
$Δ G = Δ H - T Δ S$
and for a spontaneous reaction,
$Δ G = - v e$
which happens only at higher temperature.

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Similar questions

A change in the free energy of a system at constant temperature and pressure will be:

Δ_{s y s} G = Δ_{s y s} H - T Δ_{s y s} S

At constant temperature and pressure,

Δ_{s y s} G < 0 (s p o n t a n e o u s)

Δ_{s y s} G = 0 (e q u i l i b r i u m)

Δ_{s y s} G > 0 (n o n - s p o n t a n e o u s)

A reaction has positive values of

Δ H

Δ S

From this you can deduce that the reaction:

Q. A reaction has

Δ H = - 33 kJ

Δ S = - 58 J/K

. This reaction would be:

Q. Suppose a reaction has

Δ H = - 40 k J

Δ S = - 50 J / K

. At what temperature range will reaction become spontaneous from non-spontaneous?

Q. Suppose that a reaction has

Δ H = 40 k J

Δ S = 50 k J / K

. At what temperature range will it change from spontaneous to non-spontaneous?

A reaction will never be spontaneous at any temperature and pressure provided.

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