Assertion : Delta H and Delta E are almost sa | vedclass

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(B) The relationship between enthalpy change and internal energy change is given by $\Delta H = \Delta E + \Delta n_g RT$.For the reaction $N_{2(g)} +

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

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(B) The relationship between enthalpy change and internal energy change is given by $\Delta H = \Delta E + \Delta n_g RT$.For the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$,the change in the number of moles of gaseous species is $\Delta n_g = 2 - (1 + 1) = 0$.Since $\Delta n_g = 0$,we have $\Delta H = \Delta E$.Thus,the Assertion is correct.The Reason states that all reactants and products are gases,which is true,but this alone does not guarantee $\Delta H = \Delta E$. The equality holds only because $\Delta n_g = 0$. Therefore,the Reason is not the correct explanation for the Assertion.

List-$I$	List-$II$
$A$. Spontaneous process	$I$. $\Delta H < 0$
$B$. Process with $\Delta P = 0; \Delta T = 0$	$II$. $\Delta G_{T, P} < 0$
$C$. $\Delta H_{reaction}$	$III$. Isothermal and isobaric process
$D$. Exothermic process	$IV$. [Bond energies of molecules in reactants] - [Bond energies of product molecules]

Assertion : $\Delta H$ and $\Delta E$ are almost same for the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$.
Reason : All reactants and products are gases.

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Assertion : $\Delta H$ and $\Delta E$ are almost same for the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$.Reason : All reactants and products are gases.