If the heat of combustion of isobutane at con | vedclass

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

Vedclass · Accepted Answer

$Q_v - 3.5RT$

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(A) 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,$\Delta H$ represents the heat of combustion at constant pressure $(Q_p)$ and $\Delta U$ represents the heat of combustion at constant volume $(Q_v)$.Substituting these into the equation: $Q_p = Q_v + \Delta n_g RT$.Given that $\Delta n_g = -3.5$,the equation becomes: $Q_p = Q_v - 3.5RT$.

If the heat of combustion of isobutane at constant volume is $Q_v$,what will be the heat of combustion of one mole of isobutane at constant pressure and standard conditions? (Given: $\Delta n_g = -3.5$)

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