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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 + P\D

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$(i)$ and $(iv)$

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(A) The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta U)$ is given by the equation: $\Delta H = \Delta U + P\Delta V$.For solids and liquids, the change in volume $(\Delta V)$ is extremely small, making the term $P\Delta V$ negligible.Therefore, for solids and liquids, $\Delta H \approx \Delta U$.In contrast, for gases, $\Delta V$ is significant, and $P\Delta V = \Delta n_g RT$, which is not negligible.Thus, the difference is not significant for $(i)$ Solids and $(iv)$ Liquids.

For which of the following systems, the difference between $\Delta H$ and $\Delta U$ is not significant?
$(i)$ Solids
$(ii)$ Gases
$(iii)$ Mixture of gases and liquids
$(iv)$ Liquids

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For which of the following systems, the difference between $\Delta H$ and $\Delta U$ is not significant?$(i)$ Solids$(ii)$ Gases$(iii)$ Mixture of gases and liquids$(iv)$ Liquids