Which of the following is a correct statement | vedclass

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(B) $1$. Internal energy $(U)$ and entropy $(S)$ depend only on the state of the system, not on the path taken to reach that state, hence they are sta

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Internal energy and entropy are state functions

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(B) $1$. Internal energy $(U)$ and entropy $(S)$ depend only on the state of the system, not on the path taken to reach that state, hence they are state functions.$2$. Work $(w)$ and heat $(q)$ are path functions, not state functions.$3$. Internal energy does not change in an isothermal process for an ideal gas $(\Delta U = 0)$.$4$. Work done in an adiabatic process is not necessarily zero; it is given by $w = \Delta U$.

Which of the following is a correct statement for a thermodynamic system?

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