The P-V diagram of a system undergoing a ther | vedclass

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

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$10$

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(A) According to the first law of thermodynamics,the heat supplied to a system $(\Delta Q)$ is equal to the sum of the change in internal energy $(\Delta U)$ and the work done by the system $(\Delta W)$: $\Delta Q = \Delta U + \Delta W$ Given: Heat supplied,$\Delta Q = 40 \ J$ Work done,$\Delta W = 30 \ J$ Substituting these values into the equation: $40 \ J = \Delta U + 30 \ J$ $\Delta U = 40 \ J - 30 \ J = 10 \ J$ Therefore,the change in internal energy between $A$ and $C$ is $10 \ J$.

The $P-V$ diagram of a system undergoing a thermodynamic transformation is shown in the figure. The work done by the system in going from $A \to B \to C$ is $30 \ J$ and $40 \ J$ of heat is given to the system. The change in internal energy between $A$ and $C$ is ....... $J$.

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