When $1 \, mol$ of nitrogen gas is heated at constant pressure at room temperature,it is supplied with $1163.4 \, J$ of energy. The increase in temperature is ....... $K$ $(R = 8.31 \, J \, mol^{-1} \, K^{-1})$.

$A$ cyclic process of a thermodynamic system is taken through $a \to b \to c \to d \to a$ as shown in the $P-V$ diagram. The work done by the gas along the path $b \to c$ is

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?

Which one of the following equations specifies an isobaric process?
$[Q=$ heat supplied; $\Delta P, \Delta V$ and $\Delta T$ are change in pressure,volume,and temperature respectively.]

$A$ 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 ............ $J$.

$A$ frictionless piston-cylinder based enclosure contains some amount of gas at a pressure of $400 \text{ kPa}$. Heat is transferred to the gas at constant pressure in a quasi-static process. The piston moves up slowly through a height of $10 \text{ cm}$. If the piston has a cross-sectional area of $0.3 \text{ m}^2$, the work done by the gas in this process is: (in $\text{ kJ}$)