Assertion: The heat supplied to a system is a | vedclass

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(D) According to the first law of thermodynamics,$\Delta Q = \Delta U + \Delta W = \Delta U + P\Delta V$.If heat is supplied in such a manner that the

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If both the $Assertion$ and $Reason$ are incorrect.

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(D) According to the first law of thermodynamics,$\Delta Q = \Delta U + \Delta W = \Delta U + P\Delta V$.If heat is supplied in such a manner that the volume does not change $(\Delta V = 0)$,i.e.,an isochoric process,then the whole of the heat energy supplied to the system will increase the internal energy only.However,in any other process where work is done,the heat supplied is distributed between the change in internal energy and the work done by the system.Therefore,the $Assertion$ is incorrect.The $Reason$ is also incorrect because when a system changes from one thermal equilibrium to another,heat may be absorbed,evolved,or remain zero depending on the process.

$Assertion:$ The heat supplied to a system is always equal to the increase in its internal energy.
$Reason:$ When a system changes from one thermal equilibrium to another,some heat is absorbed by it.

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$Assertion:$ The heat supplied to a system is always equal to the increase in its internal energy.$Reason:$ When a system changes from one thermal equilibrium to another,some heat is absorbed by it.