For which of the following reactions is Delta | vedclass

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(B) 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

$N_2(g) + O_2(g) 	o 2NO(g)$

Vedclass · Answer

(B) 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 $\Delta H = \Delta E$ to hold true,the change in the number of moles of gaseous products and reactants must be zero,i.e.,$\Delta n_g = 0$. In option $B$,$N_2(g) + O_2(g) 	o 2NO(g)$,the number of moles of gaseous products is $2$ and the number of moles of gaseous reactants is $1 + 1 = 2$. Thus,$\Delta n_g = 2 - 2 = 0$. Therefore,$\Delta H = \Delta E + (0)RT = \Delta E$.

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

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