Which of the following statements is correct | vedclass

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(B) Internal energy is a state function,meaning it depends only on the state of the system and not on the path taken. Similarly,entropy is also a stat

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Internal energy and entropy are state functions.

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(B) Internal energy is a state function,meaning it depends only on the state of the system and not on the path taken. Similarly,entropy is also a state function. In an isothermal process,the temperature remains constant,and for an ideal gas,the internal energy does not change $(\Delta U = 0)$. In a reversible adiabatic process,the entropy change is zero $(\Delta S = 0)$. Work done in an adiabatic process is given by $W = -\Delta U$,which is generally non-zero. Therefore,the statement that internal energy and entropy are state functions is correct.

List-$I$	List-$II$
$(i) \ a \bar{a}$	$(A) -\frac{\pi}{3}$
$(ii) \ \arg \left(\frac{1}{\bar{a}}\right)$	$(B) -i \sqrt{3}$
$(iii) \ a-\bar{a}$	$(C) \frac{2i}{\sqrt{3}}$
$(iv) \ \operatorname{Im}\left(\frac{4}{3a}\right)$	$(D) 1$
	$(E) \frac{\pi}{3}$
	$(F) \frac{2}{\sqrt{3}}$

Which of the following statements is correct for any thermodynamic system?

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