$1 \text{ mole}$ of an ideal gas is compressed isothermally and reversibly from an initial pressure $x \text{ kPa}$ to a final pressure $2x \text{ kPa}$ at $300 \text{ K}$. Find the work done $(R = 8.314 \text{ J K}^{-1} \text{mol}^{-1})$. (in $\text{ J}$)

The process,in which no heat enters or leaves the system,is termed as

What is the work done when a gas is compressed from $2.5 \times 10^{-2} \ m^3$ to $1.3 \times 10^{-2} \ m^3$ at a constant external pressure of $4.05 \ bar$ (in $J$)?

$A$ gas expands from a volume of $1 \ m^{3}$ to a volume of $2 \ m^{3}$ against an external pressure of $10^{5} \ Nm^{-2}$. The work done by the gas will be

$X$ is an extensive property and $x$ is an intensive property of a thermodynamic system. Which of the following statement$(s)$ is (are) correct?

Fill in the blanks:
$(i)$ The process of attaining thermal equilibrium between any two heat-conducting bodies is called the $\dots\dots$ law of thermodynamics.
$(ii)$ The law of thermodynamics is actually the law of $\dots\dots$.
$(iii)$ $A$ thermometer measures temperature according to the $\dots\dots$ law of thermodynamics.