Assertion : In an isothermal process,the whol | vedclass

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(D) The first law of thermodynamics is given by $\Delta Q = \Delta U + P\Delta V$.For an ideal gas,the internal energy $U$ is a function of temperatur

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If both the Assertion and Reason are incorrect.

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(D) The first law of thermodynamics is given by $\Delta Q = \Delta U + P\Delta V$.For an ideal gas,the internal energy $U$ is a function of temperature $T$ only $(U = f(T))$.In an isothermal process,the temperature remains constant,so $\Delta T = 0$.Since $\Delta U = nC_v\Delta T$,it follows that $\Delta U = 0$ for an isothermal process.Substituting this into the first law: $\Delta Q = 0 + P\Delta V$,which means $\Delta Q = P\Delta V$.Therefore,the heat supplied is converted into work done by the system,not internal energy.Thus,the Assertion is incorrect,and the Reason is a correct statement of the first law of thermodynamics.

$Assertion :$ In an isothermal process,the whole of the heat supplied to the body is converted into internal energy.
$Reason :$ According to the first law of thermodynamics,$\Delta Q = \Delta U + P\Delta V$.

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$Assertion :$ In an isothermal process,the whole of the heat supplied to the body is converted into internal energy.$Reason :$ According to the first law of thermodynamics,$\Delta Q = \Delta U + P\Delta V$.