Assertion :For a reaction at equilibrium, the Gibb's free energy of reaction is minimum at constant temp. and pressure. Reason: The Gibb's free energy of both reactants and products increases and become equal at equilibrium.

Both Assertion and Reason are correct and Reason is the correct explanation for Assertion

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Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion

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Assertion is correct but Reason is incorrect

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Assertion is incorrect but Reason is correct

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Solution

The correct option is D Assertion is incorrect but Reason is correct
For a reaction at equilibrium, Gibb's free energy change of the reaction is zero at constant temperature and pressure.
The Gibb's free energy of both reactants and products increases and become equal at equilibrium.
Hence, Assertion is incorrect but Reason is correct

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Similar questions

Assertion (A) The enthalpy of reaction remains constant in the presence of a catalyst.

Reason (R) A catalyst participating in the reaction forms different activated complex and lowers down the activation energy but the difference in enrgy of reactant and product remains the same.

(a) Both assertion and reason are correct and the reason is correct explanation of assertion
(b) Both assertion and reason are correct, but reason does not explain assertion.
(c) Assertion is correct, but reason is incorrect
(d) Both assertion and reason are incorrect
(e) Assertion is incorrect but reason is correct.

Q. Assertion :For a reaction at equilibrium,the Gibb's free energy of reaction is minimum at constant temperature and pressure. Reason: The Gibb's free energy of both reactants and products increases and become equal at equilibrium.

Read the above assertion and reason and choose the correct option regarding it.

Q. Assertion: The compressibility factor for