Discussion
For the isothermal expansion of an ideal gas in a piston cylinder system, the net heat supplied during the process is equal to the net work. Which one of the following statements is correct for the given process?
Answer: A
The process is possible.
For an ideal gas the internal energy depends only on temperature, so in an isothermal process \(\Delta U = 0\). The first law then gives \(Q = W\): all the heat supplied is converted into expansion work. That is exactly what the question describes.
This does not violate the second law, which forbids a cycle converting heat completely into work; a single non-cyclic process such as this expansion can do so, because the gas ends in a different state. So the options claiming a violation of either law are wrong.
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