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Urvashi Kartik Khan
Asked: 2022-11-04T18:30:11+05:30 In:

Assertion (A): For every chemical reaction at equilibrium, standard Gibbs enegry of the reaction is zero.
Reason (R ) : At constant temperature and pressure chemical reactions are spontaneous in the direction of the decreasing Gibbs energy.
A. Both (A) and (R ) are correct, and (R ) is the correct explanation for (A).
B. Both (A) and (R ) are correct, but(R ) is not a correct explanation for (A).
C. (A) is correct, but (R ) is incorrect.
D. (A) is incorrect, but (R ) is correct.

Assertion (A): For every chemical reaction at equilibrium, standard Gibbs enegry of the reaction is zero.
Reason (R ) : At constant temperature and pressure chemical reactions are spontaneous in the direction of the decreasing Gibbs energy.
A. Both (A) and (R ) are correct, and (R ) is the correct explanation for (A).
B. Both (A) and (R ) are correct, but(R ) is not a correct explanation for (A).
C. (A) is correct, but (R ) is incorrect.
D. (A) is incorrect, but (R ) is correct.
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  1. (A) is false, (R ) is true.
    For every chemical reaction at equilibrium standard Gibbs energy of the reaction is not zero. It is zero only for the reactions at equilibrium. At constant temperature and pressure, the chemical reactions are spontaneous in the direction of the decreasing Gibbs energy. For a reaction to be spontaneous, the free energy should decreases.

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Mitesh Chandra Mander
Asked: 2022-10-31T22:33:16+05:30 In:

Assertion (A): For every chemical reaction at equilibrium, standard Gibbs enegry of the reaction is zero.
Reason (R ) : At constant temperature and pressure chemical reactions are spontaneous in the direction of the decreasing Gibbs energy.
A. statement I is true, Statement II is true, Statement II is the correct explanation of Statement I
B. Statement I is true , statement II is true , Statement II is not the correct explanation of Statement I
C. Statement I is true, Statement II is false
D. Statement I is false, Statement II is true

Assertion (A): For every chemical reaction at equilibrium, standard Gibbs enegry of the reaction is zero.
Reason (R ) : At constant temperature and pressure chemical reactions are spontaneous in the direction of the decreasing Gibbs energy.
A. statement I is true, Statement II is true, Statement II is the correct explanation of Statement I
B. Statement I is true , statement II is true , Statement II is not the correct explanation of Statement I
C. Statement I is true, Statement II is false
D. Statement I is false, Statement II is true
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  1. Correct Answer – d

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Naina Ishat Zacharia
Asked: 2022-10-29T23:31:04+05:30 In:

Assertion (A): For every chemical reaction at equilibrium, standard Gibbs enegry of the reaction is zero.
Reason (R ) : At constant temperature and pressure chemical reactions are spontaneous in the direction of the decreasing Gibbs energy.
A. `S` is correct but `E` is wrong.
B. `S` is wrong but `E` are correct and `E`
C. Both `S` and `E` are correct but `E` is correct explanation of `S`.
D. Both `S` and `E` are correct but `E` is not correct explanation of `S`.

Assertion (A): For every chemical reaction at equilibrium, standard Gibbs enegry of the reaction is zero.
Reason (R ) : At constant temperature and pressure chemical reactions are spontaneous in the direction of the decreasing Gibbs energy.
A. `S` is correct but `E` is wrong.
B. `S` is wrong but `E` are correct and `E`
C. Both `S` and `E` are correct but `E` is correct explanation of `S`.
D. Both `S` and `E` are correct but `E` is not correct explanation of `S`.
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  1. Correct Answer – b
    AT equilibrium `DeltaG=0`, but standard Gibbs energy `(DeltaG^(2))` of a reaction may or may not be zero. For reaction to be spontaneousn `DeltaG`(Gibbs energy) should be more negative, i.e., `DeltaGgt0`.

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