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(C) The enthalpy change $(\Delta H)$ is defined as the change in internal energy $(\Delta U)$ plus the work done due to volume change at constant pres

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$\Delta H = \Delta U + \Delta n_{g} R T$

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(C) The enthalpy change $(\Delta H)$ is defined as the change in internal energy $(\Delta U)$ plus the work done due to volume change at constant pressure.For a chemical reaction involving gases,the relation is given by:$\Delta H = \Delta U + \Delta n_{g} R T$Where:$\Delta H$ = Change in enthalpy$\Delta U$ = Change in internal energy$\Delta n_{g}$ = Change in the number of moles of gaseous products and reactants$R$ = Universal gas constant$T$ = Temperature in Kelvin

Which amongst the following options is the correct relation between change in enthalpy and change in internal energy?

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