During the isothermal expansion,a confined id | vedclass

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(B) For an isothermal process,the change in internal energy $(\Delta U)$ is $0$ because the temperature remains constant.According to the First Law of

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$150 \ J$ of heat has been removed from the gas

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(B) For an isothermal process,the change in internal energy $(\Delta U)$ is $0$ because the temperature remains constant.According to the First Law of Thermodynamics,$\Delta Q = \Delta U + W$.Here,the work done by the gas is $W = -150 \ J$ (as the gas does work against the surroundings,the system loses energy).Substituting the values into the equation: $\Delta Q = 0 + (-150 \ J) = -150 \ J$.$A$ negative sign for $\Delta Q$ indicates that heat is removed from the system.Therefore,$150 \ J$ of heat has been removed from the gas.

During the isothermal expansion,a confined ideal gas does $(-150) \ J$ of work against its surroundings. This means that

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