In a thermodynamic process, pressure of a fixed mass of a...

In a thermodynamic process, pressure of a fixed mass of a gas is changed in such a manner that the gas release $20 \mathrm{~J}$ of heat and $8 \mathrm{~J}$ of work has done on the gas-If the initial internal energy of the gas was $30 \mathrm{j}$, then the final internal energy will be (A) $58 \mathrm{~J}$ (B) $2 \mathrm{~J}$ (C) $42 \mathrm{~J}$ (D) $18 \mathrm{~J}$

In a thermodynamic process, pressure of a fixed mass of a gas is changed in such a manner that the gas release $20 \mathrm{~J}$ of heat and $8 \mathrm{~J}$ of work has done on the gas-If the initial internal energy of the gas was $30 \mathrm{j}$, then the final internal energy will be
(A) $58 \mathrm{~J}$
(B) $2 \mathrm{~J}$
(C) $42 \mathrm{~J}$
(D) $18 \mathrm{~J}$

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Key Concepts

First Law of Thermodynamics

This law states that the change in the internal energy of a system is equal to the heat added to the system plus the work done on the system. It encapsulates the principle of conservation of energy in thermodynamic processes and is essential for analyzing energy transfers during chemical and physical changes.

Sign Conventions in Thermodynamics

Understanding sign conventions is crucial in thermodynamics, as heat and work can either be added to or removed from a system. Typically, heat added to the system is taken as positive, while heat removed is negative; similarly, work done on the system is positive and work done by the system is negative. This convention ensures that energy transfers are consistently applied when using the first law.

Internal Energy

Internal energy refers to the total energy contained within a system, including both kinetic and potential energies of the molecules. Changes in internal energy result from heat transfers and work interactions, making it a key concept for understanding the state and evolution of a thermodynamic system.

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