If Delta U and Delta W represent the increase | vedclass

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(B) According to the first law of thermodynamics,$Q = \Delta U + \Delta W$,where $Q$ is the heat supplied to the system,$\Delta U$ is the change in in

Vedclass · Accepted Answer

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

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(B) According to the first law of thermodynamics,$Q = \Delta U + \Delta W$,where $Q$ is the heat supplied to the system,$\Delta U$ is the change in internal energy,and $\Delta W$ is the work done by the system.In an adiabatic process,there is no exchange of heat between the system and the surroundings,so $Q = 0$.Substituting $Q = 0$ into the first law equation: $0 = \Delta U + \Delta W$.Rearranging the terms,we get $\Delta U = -\Delta W$.Therefore,the correct statement is that in an adiabatic process,the increase in internal energy is equal to the negative of the work done by the system.

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

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