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Assertion: For a reaction 2NH3(g) → N2(g) + 3H2(g); ΔH > ΔE Reason : Enthalpy change is always greater than internal energy change.

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Assertion: For a reaction

2NH3(g) → N2(g) + 3H2(g); ΔH > ΔE

Reason : Enthalpy change is always greater than internal energy change.

(a) If both Assertion and Reason are correct and the Reason is a correct explanation of the Assertion.

(b) If both Assertion and Reason are correct but Reason is not a correct explanation of the Assertion.

(c) If the Assertion is correct but Reason is incorrect.

(d) If both the Assertion and Reason are incorrect.

(e) If the Assertion is incorrect but the Reason is correct.

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(c) If the Assertion is correct but Reason is incorrect.

Explanation:

For given reaction ΔH > ΔE because {ΔH = ΔE + ΔnRT}. In this reaction Δn(g) is [(3 + 1) - 2 = +2] so ΔH > ΔE.

Thus, assertion is true. In some cases, the enthalpy change may be less than internal energy change (in these cases Δn(g), is negative), so the reason is false.

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