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 $R$)

When an ideal gas $\left(\gamma = \frac{5}{3}\right)$ is heated under constant pressure,then what percentage of given heat energy will be utilised in doing external work (in $\%$)?

In an isobaric process,the work done by a diatomic gas is $10 \ J$. The heat given to the gas will be (in $J$):

The work done by $6$ moles of helium gas when its temperature increases by $20^{\circ} C$ at constant pressure is (Universal gas constant $R = 8.31 \ J \ mol^{-1} \ K^{-1}$) (in $J$)

Work done by air when it expands from $50 \, L$ to $150 \, L$ at a constant pressure of $2 \, atm$ is:

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 $:-$