In an isobaric process,

$A$ container having $1$ mole of a gas at a temperature $27^{\circ}C$ has a movable piston which maintains a constant pressure in the container of $1 \, atm$. The gas is compressed until the temperature becomes $127^{\circ}C$. The work done is ........ $J$ ($C_P$ for the gas is $7.03 \, cal/mol-K$).

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 $J$)

Two cylinders contain the same amount of an ideal monatomic gas. The same amount of heat is given to both cylinders. If the temperature rise in cylinder $A$ is $T_0$,then the temperature rise in cylinder $B$ will be:

When an ideal gas $(\gamma = 5/3)$ is heated under constant pressure,what percentage of the given heat energy will be utilized in doing external work (in $\%$)?

The condition $dQ = dU$ (heat supplied equals the increase in internal energy) is true for which of the following processes?