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Byju's Answer
Standard XII
Chemistry
System, Surroundings, Intensive, Extensive Properties
Δ total S<0
Question

ΔtotalS<0
  1. 0

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Solution

The correct option is A 0
As we know,
for a spontaneous process,
ΔG=ΔH−TΔS<0
and
ΔtotalS>0

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Q.
State True or False.
At equilibrium state ΔtotalS=0
Q. For a spontaneous process, which of the following is always true :

a. ΔG>0 b. ΔtotalS<0 c. TΔS>0 d. ΔG<0

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.
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. 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:

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