ASSERTION(A): For every chemical reaction at equilibrium, standard Gibbs energy of the reaction is zero.
REASON(R): At constant temperature and pressure, chemical reactions are spontaneous in the direction of the decreasing Gibbs energy.

If both (A) and (R) are correct, and (R) is the correct explanation for (A)

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If the both (A) and (R) are correct, but (R) is not the correct explanation for (A)

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If (A) is correct, but (R) is incorrect

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IF (A) is incorrect, but (R) is correct

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Solution

The correct option is D
IF (A) is incorrect, but (R) is correct

Don't get confused in the question here. During equilibrium, $△ G^{⊖}$ = 0 Standard Gibbs energy of the reaction is not zero.
And for the second statement,
It is given reaction is spontaneous.
Therefore, $△ G$ = -ve
$G_{f i n a l} - G_{i n i t i a l}$ = -ve
Therefore, $G_{f i n a l}$ < $G_{i n i t i a l}$
So, this statement is correct.

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Similar questions

ASSERTION(A): For every chemical reaction at equilibrium, standard Gibbs energy of the reaction is zero.
REASON(R): At constant temperature and pressure, chemical reactions are spontaneous in the direction of the decreasing Gibbs energy.

Q. Assertion: For every chemical reaction at equilibrium, the standard Gibbs energy of reaction is zero.
Reason: At constant temperature and pressure, chemical reactions are spontaneous in the direction of decreasing Gibbs energy.

Q. Select the correct statements.
a. There is asymmetry between converting work to heat and converting heat to work.
b. No process is possible in which the sole result is the absorption of heat from a reservoir and its complete conversion into work.
c. For every chemical reaction at equilibrium, standard change in Gibbs free energy is zero.
d. At constant temperature and pressure, chemical reactions are spontaneous in the direction of decreasing Gibbs energy.

Q. The standard reaction Gibbs energy for a chemical reaction at an absolute temperature T is given

△_{r} G^{\circ} = A - B T,

where A and B are non-zero constants. Which of the following is true about this reaction?

Q. The standard reaction Gibbs energy for a chemical reaction at an absolute temperature

T

is given by:

Δ_{r} G^{o} = A - B T

Where

A

and

B

are non-zero constants. Which of the following is true about this reaction?

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ASSERTION(A): For every chemical reaction at equilibrium, standard Gibbs energy of the reaction is zero. REASON(R): At constant temperature and pressure, chemical reactions are spontaneous in the direction of the decreasing Gibbs energy.

ASSERTION(A): For every chemical reaction at equilibrium, standard Gibbs energy of the reaction is zero.
REASON(R): At constant temperature and pressure, chemical reactions are spontaneous in the direction of the decreasing Gibbs energy.