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Standard XII
Chemistry
Gibbs Free Energy & Spontaneity
For a spontan...
Question

For a spontaneous process, which of the following is always true :


a. ΔG>0 b. ΔtotalS<0 c. TΔS>0 d. ΔG<0

A
a
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B
b
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C
c
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D
d
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Solution

The correct option is D d
As we know,

for a spontaneous process,

ΔG=ΔH−TΔS<0

and

ΔtotalS>0

Hence, option D is correct.

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Q. Free energy, G=H−TΔS, is a state function that indicates whether a reaction is spontaneous or non-spontaneous. If you think of TS as the part of the system`s energy that is disordered already, then (H−TS) is the part of the system`s energy that is still ordered and therefore free to cause spontaneous change by becoming disordered.
Also, ΔG=ΔH−TΔS
From the second law of thermodynamics, a reaction is spontaneous if ΔtotalS is positive, non-spontaneous if ΔtotalS is negative, and at equilibrium if ΔtotalS is zero.
Since −TΔS=ΔG and since ΔG and ΔS have opposite signs, we can restate the Thermodynamic criterion for the spontaneity of a reaction carried out at a constant temperature and pressure.
If ΔG<0, the reaction is spontaneous
If ΔG>0, the reaction is non-spontaneous
If ΔG=0, the reaction is at equilibrium
Read the above paragraph carefully and answer the following questions based on the above comprehension.
Which of the following is correct?

Q. Free energy, G=H−TΔS, is a state function that indicates whether a reaction is spontaneous or non-spontaneous. If you think of TS as the part of the system`s energy that is disordered already, then (H−TS) is the part of the system`s energy that is still ordered and therefore free to cause spontaneous change by becoming disordered.
Also, ΔG=ΔH−TΔS
From the second law of Thermodynamics, a reaction is spontaneous if ΔtotalS is positive, non-spontaneous if ΔtotalS is negative, and at equilibrium if ΔtotalS is zero.
Since, −TΔS=ΔG and since ΔG and ΔS have opposite signs, we can restate the Thermodynamic criterion for the spontaneity of a reaction carried out at a constant temperature and pressure.
If ΔG<0, the reaction is spontaneous
If ΔG>0, the reaction is non-spontaneous
If ΔG=0, the reaction is at equilibrium
Read the above paragraph carefully and answer the following questions based on the above comprehension.
If an endothermic reaction is non-spontaneous at freezing point of water and becomes feasible at its boiling point, then:

Q. Free energy, G=H−TΔS, is a state function that indicates whether a reaction is spontaneous or non-spontaneous. If you think of TS as the part of the system`s energy that is disordered already, then (H−TS) is the part of the system`s energy that is still ordered and therefore free to cause spontaneous change by becoming disordered.
Also, ΔG=ΔH−TΔS
From the second law of Thermodynamics, a reaction is spontaneous if ΔtotalS is positive, non-spontaneous if ΔtotalS is negative, and at equilibrium if ΔtotalS is zero.
Since, −TΔS=ΔG and since ΔG and ΔS have opposite signs, we can restate the Thermodynamic criterion for the spontaneity of a reaction carried out at a constant temperature and pressure.
If ΔG<0, the reaction is spontaneous
If ΔG>0, the reaction is non-spontaneous
If ΔG=0, the reaction is at equilibrium
Read the above paragraph carefully and answer the following questions based on the above comprehension.
One mol of ice is converted to liquid at 273K; H2O(s) and H2O(l) have entropies 38.20 and 60.03Jmol−1dg−1. Enthalpy change in the conversion will be:

Q. From application of thermodynamics on chemical reaction,
we get ΔG=ΔG0+RT ln Q
Also ΔG=ΔH−TΔS.
If ΔG=0, reaction is at equilibrium.
If ΔG>0 reaction is non-spontaneous under given condition. IfΔG<0, reaction is spontaneous under given condition.
Consider the reaction given below.
A(s)⇌2B(g) ΔH0=160 KJ/mol.
ΔS0=400 J/mol-K at 400 K
Which of the following is correct at 400 K?

Q. ΔG=ΔH−TΔS.

If true enter 1, else enter 0.
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