Which is not the correct relation between ent | vedclass

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Question

(C) The fundamental relation between enthalpy $(\Delta H)$ and internal energy $(\Delta E)$ for a process at constant pressure is given by $\Delta H =

Vedclass · Accepted Answer

$\Delta H = \Delta E - P \Delta V$

Vedclass · Answer

(C) The fundamental relation between enthalpy $(\Delta H)$ and internal energy $(\Delta E)$ for a process at constant pressure is given by $\Delta H = \Delta E + P \Delta V$. Rearranging this equation gives $\Delta E = \Delta H - P \Delta V$. For gaseous reactions,the work done $P \Delta V$ is equivalent to $\Delta n_g RT$,where $\Delta n_g$ is the change in the number of moles of gaseous species. Thus,$\Delta H = \Delta E + \Delta n_g RT$ (often written as $\Delta H = \Delta E + n RT$). Therefore,the relation $\Delta H = \Delta E - P \Delta V$ is incorrect.

Which is not the correct relation between enthalpy $(\Delta H)$ and internal energy $(\Delta E)$?

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