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(A) According to the first law of thermodynamics,$\Delta U = q + w$. For an isobaric process (constant pressure),the heat exchanged is $q_p = \Delta H

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For an isobaric process,$q_p = \Delta U + w$

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(A) According to the first law of thermodynamics,$\Delta U = q + w$. For an isobaric process (constant pressure),the heat exchanged is $q_p = \Delta H = \Delta U + P\Delta V$. Since work done $w = -P\Delta V$,we have $P\Delta V = -w$. Substituting this,$q_p = \Delta U - w$,which means $\Delta U = q_p + w$. Thus,option $A$ is correct. For an adiabatic process,$q = 0$,so $\Delta U = w$. For an isochoric process,$\Delta V = 0$,so $w = 0$ and $\Delta U = q_v$. For an isothermal process of an ideal gas,$\Delta U = 0$,so $q = -w$.

Based on the first law of thermodynamics,which of the following is correct?

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