An ideal monoatomic gas of $1.5$ moles is heated at a constant pressure of $2 \,atm$ so that its temperature increases from $30^{\circ} C$ to $130^{\circ} C$. The work done by the gas is (Universal gas constant $R = 8.3 \,J \,mol^{-1} \,K^{-1}$). (in $\,J$)

An ideal gas goes from an initial state to a final state. During the process,the pressure of the gas increases linearly with temperature. Which of the following statements are correct?
$A.$ The work done by the gas during the process is zero.
$B.$ The heat added to the gas is different from the change in its internal energy.
$C.$ The volume of the gas is increased.
$D.$ The internal energy of the gas is increased.
$E.$ The process is isochoric (constant volume process).
Choose the correct answer from the options given below $:-$

$A$ sample of gas expands from volume ${V_1}$ to ${V_2}$. The amount of work done by the gas is greatest when the expansion is

Two moles of ideal helium gas are in a rubber balloon at $30^{\circ} C$. The balloon is fully expandable and can be assumed to require no energy in its expansion. The temperature of the gas in the balloon is slowly changed to $35^{\circ} C$. The amount of heat required in raising the temperature is nearly (take $R = 8.31 \ J / mol \cdot K$) (in $J$)

$A$ diatomic gas $(\gamma = 1.4)$ does $400 \ J$ of work when it is expanded isobarically. The heat given to the gas in the process is ............ $J$.

$A$ gas expands by $0.25 \ m^{3}$ at a constant pressure of $10^{3} \ N/m^{2}$. Calculate the work done.