An ideal gas undergoes a cyclic process as shown in the diagram. The net work done by the gas in the cycle is

An ideal gas is made to undergo the cyclic process shown in the figure below. Let $\Delta W$ depict the work done,$\Delta U$ be the change in internal energy of the gas,and $Q$ be the heat added to the gas. The signs of each of these three quantities for the whole cycle will be ($0$ refers to no change):

One mole of a monatomic ideal gas undergoes the process $A \rightarrow B$ in the given $p-V$ diagram. The specific heat capacity in the process is:

$3\, \text{moles}$ of an ideal monoatomic gas perform a cycle as shown in the figure. The gas temperatures in different states are: $T_1 = 400\, K$, $T_2 = 800\, K$, $T_3 = 2400\, K$ and $T_4 = 1200\, K$. The work done by the gas during the cycle is ...... $kJ$.

One mole of a gas obeying the equation of state $P(V-b)=RT$ is made to expand from a state with coordinates $(P_{1}, V_{1})$ to a state with $(P_{2}, V_{2})$ along a process that is depicted by a straight line on a $P-V$ diagram. Then, the work done is given by

$A$ quantity of monoatomic gas undergoes a process in which pressure is changed linearly with volume. The pressure and volume are changed from initial value $(P_{o}, V_{o})$ to final value $(3 P_{o}, 3 V_{o})$. The heat absorbed by the gas during the process is (in $P_{o} V_{o}$)