One mole of a diatomic gas is heated at constant pressure starting at $ 27^{\circ}C $. How much energy must be added to the gas as heat to double its volume?

For an isochoric process,if $T_1 = 27 \, ^\circ C$ and $T_2 = 127 \, ^\circ C$,then $P_1 / P_2 = \dots$

$A$ diatomic gas $(\gamma = 1.4)$ does $100 \ J$ of work when it is expanded isobarically. Then the heat given to the gas is . . . . . . $J$.

Find the heat energy required to increase the temperature of $2$ moles of a monoatomic gas from $273 \ K$ to $373 \ K$. (No work is done in the process.) (in $R$)

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.

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 $R$)