For which of the following reactions is Delta | vedclass

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(C) The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta E)$ is given by the equation: $\Delta H = \Delta E + \De

Vedclass · Accepted Answer

$H_{2(g)} + Cl_{2(g)} \rightleftharpoons 2HCl_{(g)}$

Vedclass · Answer

(C) The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta E)$ is given by the equation: $\Delta H = \Delta E + \Delta n_g RT$. For $\Delta H = \Delta E$,the term $\Delta n_g$ must be equal to $0$. $\Delta n_g$ is the difference between the number of moles of gaseous products and gaseous reactants. For option $C$: $H_{2(g)} + Cl_{2(g)} \rightleftharpoons 2HCl_{(g)}$,$\Delta n_g = 2 - (1 + 1) = 0$. Therefore,for this reaction,$\Delta H = \Delta E$.

For which of the following reactions is $\Delta E = \Delta H$?

Similar Questions

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