If Delta E_{int} represents the increase in i | vedclass

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(C) According to the first law of thermodynamics,the change in internal energy is given by $\Delta E_{int} = \Delta Q - W$,where $\Delta Q$ is the hea

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$\Delta E_{int} = -W$ for an adiabatic process

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(C) According to the first law of thermodynamics,the change in internal energy is given by $\Delta E_{int} = \Delta Q - W$,where $\Delta Q$ is the heat supplied to the system and $W$ is the work done by the system.For an adiabatic process,there is no exchange of heat with the surroundings,so $\Delta Q = 0$.Substituting this into the first law equation,we get $\Delta E_{int} = 0 - W$,which simplifies to $\Delta E_{int} = -W$.Therefore,the correct statement is that for an adiabatic process,the increase in internal energy is equal to the negative of the work done by the system.

If $\Delta E_{int}$ represents the increase in internal energy and $W$ represents the work done by the system,which of the following statements is correct for a thermodynamic system?

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