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Reversible Process and Change in Internal Energy

A gas undergoes a reversible isothermal compression from an initial volume of \mathrm{0.04 m^{3}} to a final volume of \mathrm{0.02 m^{3}} at a temperature of \mathrm{400 K}. If \mathrm{500 J} of heat is released to the surroundings during the process, calculate the change in internal energy of the gas

Option: 1

\mathrm{-500\: J}


Option: 2

\mathrm{700\: J}


Option: 3

\mathrm{200\: J}


Option: 4

\mathrm{220\: J}


Answers (1)

best_answer

For a reversible isothermal process, the change in internal energy \mathrm{(\Delta U)} is given by:

\mathrm{ \Delta U=Q }

Given:

\mathrm{ Q=-500 \mathrm{~J} \quad \text { (negative because heat is released) } }

The change in internal energy is equal to the heat released:

\mathrm{ \Delta U=Q=-500 \mathrm{~J} }

Therefore, the correct option is 1

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