$6$ moles of an ideal gas expand isothermally and reversibly from a volume of $1 \ L$ to a volume of $10 \ L$ at $27 \ ^oC$. What is the maximum work done? (in $kJ$)

Fill in the blanks:
$(i)$ The change in heat energy during a chemical reaction at constant volume is called .......
$(ii)$ During a ....... process,there is no absorption or evolution of heat.
$(iii)$ The equation $\Delta G = \Delta H - T \Delta S$ was proposed by .......

According to thermodynamics,when can a process be called reversible?

What will be the work done on an ideal gas enclosed in a cylinder,when it is compressed by a constant external pressure,$p_{ext}$ in a single step as shown in the figure? Explain graphically.

$A$ gas absorbs a certain amount of heat and expands by $200 \ cm^3$ against a constant external pressure of $2 \times 10^5 \ Nm^{-2}$. What is the work done by the system (in $J$)?

Which among the following pairs of properties are intensive?