For the reaction,C_2H_5OH_{(l)} + 3O_{2(g)} r | vedclass

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

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$\Delta H = \Delta U - RT$

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(D) The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta U)$ is given by the equation: $\Delta H = \Delta U + \Delta n_g RT$. Here,$\Delta n_g$ is the change in the number of moles of gaseous species. For the reaction: $C_2H_5OH_{(l)} + 3O_{2(g)} ightarrow 2CO_{2(g)} + 3H_2O_{(l)}$. $\Delta n_g = (	ext{moles of gaseous products}) - (	ext{moles of gaseous reactants}) = 2 - 3 = -1$. Substituting this value into the equation: $\Delta H = \Delta U + (-1)RT = \Delta U - RT$.

For the reaction,$C_2H_5OH_{(l)} + 3O_{2(g)} \rightarrow 2CO_{2(g)} + 3H_2O_{(l)}$,$\Delta U$ is the heat of reaction at constant volume. Then the heat of reaction at constant pressure is:

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