If $R$ is the universal gas constant,the amount of heat needed to raise the temperature of $2$ moles of an ideal monoatomic gas from $273 \ K$ to $373 \ K$ when no work is done is: (in $R$)

$A$ diatomic gas $(\gamma = 1.4)$ does $300 \ J$ of work when expanded isobarically. The heat given to the gas in this process is: (in $J$)

Which of the following relations is correct for an isochoric process?

$A$ monoatomic gas is heated at constant pressure. The percentage of total heat used for doing external work is (in $\%$)

An ideal gas undergoes the process $1 \rightarrow 2$ as shown in the figure. The heat supplied and work done in the process are $\Delta Q$ and $\Delta W$ respectively. The ratio $\Delta Q : \Delta W$ is

One mole of an ideal gas is contained within a cylinder by a frictionless piston and is initially at temperature $T$. The pressure of the gas is kept constant while it is heated and its volume doubles. If $R$ is the molar gas constant,the work done by the gas in increasing its volume is