The work done in which of the following processes is zero?

An ideal monoatomic gas expands at constant pressure. The work done by the gas on its environment is $200 \,J$, then the heat absorbed by the gas during the process is (in $\,J$)

Calculate the work done when the volume of a gas increases by $0.25\,m^3$ at a constant pressure of $10^3\,N/m^2$.

An amount of $700 \,J$ of heat is transferred to a diatomic gas, allowing it to expand with the pressure held constant. The work done by the gas is (in $\,J$)

The temperature of $3.00 \, mol$ of an ideal diatomic gas is increased by $40.0^{\circ} C$ without changing the pressure of the gas. The molecules in the gas rotate but do not oscillate. If the ratio of change in internal energy of the gas to the amount of work done by the gas is $\frac{x}{10}$,then the value of $x$ (round off to the nearest integer) is ..... . (Given $R = 8.31 \, J \, mol^{-1} K^{-1}$)

$A$ diatomic gas $(\gamma = 1.4)$ does $400 \ J$ of work when it is expanded isobarically. The heat given to the gas in the process is ............ $J$.