During an isothermal expansion,a confined ide | vedclass

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(D) According to the first law of thermodynamics,$\Delta U = Q + W$,where $\Delta U$ is the change in internal energy,$Q$ is the heat added to the sys

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$150 \, J$ of heat has been added to the gas

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(D) According to the first law of thermodynamics,$\Delta U = Q + W$,where $\Delta U$ is the change in internal energy,$Q$ is the heat added to the system,and $W$ is the work done on the system.For an isothermal process involving an ideal gas,the internal energy depends only on temperature. Since the temperature remains constant,$\Delta U = 0$.Therefore,the equation becomes $0 = Q + W$,which implies $Q = -W$.Given that the gas does work against its surroundings,the work done on the gas is $W = -150 \, J$.Substituting this value,we get $Q = -(-150 \, J) = +150 \, J$.$A$ positive value for $Q$ indicates that $150 \, J$ of heat has been added to the gas.

During an isothermal expansion,a confined ideal gas does $-150 \, J$ of work against its surroundings. This implies that

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