If Delta U and Delta W represent the increase | vedclass

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(A) According to the first law of thermodynamics,the heat supplied to the system $(\Delta Q)$ is equal to the sum of the change in internal energy $(\

Vedclass · Accepted Answer

$\Delta U = - \Delta W$ in an adiabatic process

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(A) According to the first law of thermodynamics,the heat supplied to the system $(\Delta Q)$ is equal to the sum of the change in internal energy $(\Delta U)$ and the work done by the system $(\Delta W)$: $\Delta Q = \Delta U + \Delta W$ In an adiabatic process,there is no exchange of heat with the surroundings,so $\Delta Q = 0$. Substituting $\Delta Q = 0$ into the equation,we get: $0 = \Delta U + \Delta W$ Therefore,$\Delta U = - \Delta W$.

If $\Delta U$ and $\Delta W$ represent the increase in internal energy and work done by the system respectively in a thermodynamical process,which of the following is true?

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