The pressure versus temperature (P-T) graph o | vedclass

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(C) For an ideal gas,the internal energy $U$ is a function of temperature $T$ only $(U = f(T))$.$1$. In process $AB$,the temperature $T$ is constant (

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During the process $BC$,the internal energy of the gas is increasing.

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(C) For an ideal gas,the internal energy $U$ is a function of temperature $T$ only $(U = f(T))$.$1$. In process $AB$,the temperature $T$ is constant (isochoric process in $P-V$ diagram,but here $T$ is constant,so it is an isothermal process). Since $T$ is constant,the internal energy does not change.$2$. In process $BC$,the temperature $T$ increases. Since the internal energy of an ideal gas depends only on temperature,an increase in $T$ leads to an increase in internal energy.$3$. In process $CD$,the temperature $T$ is constant (isothermal process),so the internal energy does not change.Therefore,the statement 'during the process $BC$,the internal energy of the gas is increasing' is correct.

The pressure versus temperature $(P-T)$ graph of an ideal gas is shown in the figure.

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