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Aleksandr [31]
3 years ago
9

A certain process has ΔH° > 0, ΔS° < 0, and ΔG° > 0. The values of ΔH° and ΔS° do not depend on the temperature. Which

of the following is a correct conclusion about this process? None of the above conclusions is correct. It is non-spontaneous at all T. It is spontaneous at low T. It is spontaneous at all T. It is spontaneous at high T
Chemistry
1 answer:
tino4ka555 [31]3 years ago
4 0

Answer: It is non-spontaneous at all T.

Explanation:

According to Gibb's equation:

\Delta G=\Delta H-T\Delta S

\Delta G = Gibbs free energy = +ve

\Delta H = enthalpy change  = +ve

\Delta S = entropy change  = -ve

T = temperature in Kelvin

\Delta G= +ve, reaction is non spontaneous

\Delta G= -ve, reaction is spontaneous

\Delta G= 0, reaction is in equilibrium

Putting in the values:

\Delta G=(+ve)-T(-ve)

\Delta G=(+ve)(+ve)=+ve  

Reaction is non spontaneous at all temperatures.

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Explanation:

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It is the amount of heat required to raise the temperature of one gram of substance by one degree.

Formula:

Q = m.c. ΔT

Q = amount of heat absorbed or released

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