How much work is to be done in decreasing the volume of an ideal gas by an amount of $2.4 \times 10^{-4} \ m^3$ at normal temperature and constant normal pressure of $1 \times 10^5 \ N/m^2$ (in $J$)?

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 $R$)

$A$ cylinder of fixed capacity $44.8 \ L$ contains a monatomic gas at standard temperature and pressure $(STP)$. The amount of heat required to raise the temperature of the gas in the cylinder by $10^{\circ}C$ is: ($R =$ universal gas constant)

In the figure shown,the amount of heat supplied to one mole of an ideal gas is plotted on the horizontal axis and the amount of work done by the gas is plotted on the vertical axis. Assuming the process to be isobaric,identify the gas.

$A$ certain amount of heat energy is supplied to a monoatomic ideal gas which expands at constant pressure. What fraction of the heat energy is converted into work?

The work done by a gas is maximum when it expands from a volume $V_1$ to $V_2$. This expansion is: