A piston filled with `0.04` mol of an ideal gas expands reversibly from `50.0 mL` to `375 mL` at a constant temperature of `37.0^(@)C`. As it does so, it absorbs `208 J` of heat. The value of `q` and `w` for the process will be:
`(R=8.314J//molK)(ln 7.5=2.01)`

Options

A. `q=+208J,W=-208J`
B. `q=-208J,W=-208J`
C. `q=-208J,W=+208J`
D. `q=+208J,W=+208J`

Answer

B

Explanation

As the process is carrying out at constant temperature, therefore this type of expansion is called isothermal reversible expansion, for which, `Deltamu=0` . Hence, `q=-W`
i.e., heat absorbed by the system is equal to the work done bby the system.
Thus, `q=+208J`
`W=-208J`