An ideal gas on isothermal reversible compression from $10 \ L$ to $5 \ L$ performs $1730 \ J$ of work at $300 \ K$. Calculate the number of moles of gas involved in the compression? $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

An open vessel at $27\,^{\circ}C$ is heated until two-fifths of the air (assumed as an ideal gas) in it has escaped from the vessel. Assuming that the volume of the vessel remains constant,the temperature to which the vessel has been heated is:

At a temperature of $300 \ K$,if the pressure of $0.09 \ mol$ of a gas is halved,what will be its volume?

When $48 \, L$ of dry $N_2$ gas is passed through $36 \, g$ of $H_2O$ at $27 \, ^oC$,the weight of water decreases by $1.20 \, g$. What is the vapor pressure of water in $atm$?

Calculate the new volume of a gas at constant pressure when temperature is increased to $546 \ K$.
[Initial volume of a gas at $273 \ K$ is $4 \ dm^3$] (in $dm^3$)

From the following plots,find the correct option.