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?

$A$ monoatomic ideal gas expands at constant pressure,with heat $Q$ supplied. The fraction of $Q$ which goes as work done by the gas is

The ratio of specific heats of a gas is $\gamma$. The change in internal energy of one mole of the gas, when the volume changes from $V$ to $2V$ at constant pressure $p$, is:

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 $\,J$)

In a given process for an ideal gas,$dW = 0$ and $dQ < 0$. Then for the gas:

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