NEET Chemistry Gibbs Free Energy Assertion Reason Question
Assertion (A): The standard Gibbs energy change, ΔrG°, is negative for a reaction that has an equilibrium constant Kp greater than 1. | Reason (R): A negative ΔrG° indicates that the reaction is spontaneous under standard conditions.
Both (A) and (R) are true, and (R) is the correct explanation of (A).
Both (A) and (R) are true, but (R) is not the correct explanation of (A).
(A) is true, but (R) is false.
(A) is false, but (R) is true.
Correct Answer
Detailed Explanation
The relationship ΔrG° = -RT ln Kp implies that a Kp greater than 1 results in a negative ΔrG°, indicating spontaneity, as per the NCERT context.
Found an issue with this question?
Related Questions
More from Gibbs Free Energy
More from
Using Hess's Law, calculate the standard enthalpy change for the reaction: C(graphite, s) + 2H2(g) → CH4(g), given the following reactions: 1) C(graph...
Which of the following statements about enthalpy is correct?
Which of the following statements about the First Law of Thermodynamics is correct?