An ideal monatomic gas originally in state A is taken reversibly to state B along the straight-line path shown in the pressure-volume graph.

-Suppose that the same gas is originally in state A as described above,but its volume is increased isothermally until a new volume of 3.0 liters is reached.Which one of the following statements for this isothermal process is false?

Question

An ideal monatomic gas originally in state A is taken reversibly to state B along the straight-line path shown in the pressure-volume graph.
 
-Suppose that the same gas is originally in state A as described above,but its volume is increased isothermally until a new volume of 3.0 liters is reached.Which one of the following statements for this isothermal process is false?

Quizplus · Accepted Answer

For an isothermal process involving an ideal gas, the internal energy of the gas does not change because the internal energy is a function of temperature, which remains constant in an isothermal process. This makes statement A true. The work done on the gas during an isothermal expansion is given by the formula W = nRT ln(V2/V1), where V2 > V1 for an expansion, indicating that work is done by the gas. Since the process is isothermal, the heat added to the system is equal to the work done by the system to maintain constant temperature, making statements C, D incorrect and E true. Statement B is false because changing the volume of the gas while keeping the temperature constant (isothermal process) does not guarantee that the final state will be the same as any specific state B without more information about the pressure or the specific path taken in the PV diagram.

An Ideal Monatomic Gas Originally in State a Is Taken