Consider the following statements:Statement-I | vedclass

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(D) For an ideal gas,enthalpy $(H)$ is a function of temperature only,i.e.,$H = f(T)$.In an isothermal process,the temperature remains constant $(\Del

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Statement-$I$ is not correct,but statement-$II$ is correct

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(D) For an ideal gas,enthalpy $(H)$ is a function of temperature only,i.e.,$H = f(T)$.In an isothermal process,the temperature remains constant $(\Delta T = 0)$.Therefore,the change in enthalpy $(\Delta H)$ for an ideal gas during an isothermal process is zero $(\Delta H = nC_p\Delta T = 0)$.Thus,Statement-$I$ is incorrect.For an ideal gas,internal energy $(U)$ is also a function of temperature only,i.e.,$U = f(T)$.In an isothermal process,$\Delta T = 0$,which implies $\Delta U = 0$.This holds true for expansion into vacuum (free expansion) as well.Thus,Statement-$II$ is correct.

Consider the following statements:
Statement-$I$: During isothermal expansion of an ideal gas,its enthalpy decreases.
Statement-$II$: When $2.0 \ L$ of an ideal gas expands isothermally into vacuum,$\Delta U = 0$.

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Consider the following statements:Statement-$I$: During isothermal expansion of an ideal gas,its enthalpy decreases.Statement-$II$: When $2.0 \ L$ of an ideal gas expands isothermally into vacuum,$\Delta U = 0$.