An ideal gas having pressure $P$, volume $V$, and temperature $T$ undergoes a thermodynamic process in which $dW = 0$ and $dQ < 0$. Then, for the gas

An ideal gas undergoes the process $1 \rightarrow 2$ as shown in the figure. The heat supplied and work done in the process are $\Delta Q$ and $\Delta W$ respectively. The ratio $\Delta Q : \Delta W$ is

Volume versus temperature graph of two moles of helium gas is as shown in figure. The ratio of heat absorbed and the work done by the gas in process $1-2$ is

$A$ cylinder of fixed capacity $44.8 \ L$ contains a monatomic gas at standard temperature and pressure $(STP)$. The amount of heat required to raise the temperature of the gas in the cylinder by $10^{\circ}C$ is: ($R =$ universal gas constant)

$A$ 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

An ideal diatomic gas is heated at constant pressure. The ratio of the work done to the heat supplied is