Six moles of an ideal gas perform the cycle shown in the figure. If the temperatures are $T_A = 600 \, K$, $T_B = 800 \, K$, $T_C = 2200 \, K$, and $T_D = 1200 \, K$, the work done per cycle is ........ $kJ$.

$A$ monoatomic gas is taken along path $AB$ as shown in the $V-P$ diagram. Calculate the change in internal energy of the system.

Two moles of an ideal monoatomic gas undergo a cyclic process as shown in the figure. The temperatures in different states are given as $6 T_1 = 3 T_2 = 2 T_4 = T_3 = 2400 \text{ K}$. The work done by the gas during the complete cycle is $(R = \text{Universal gas constant})$ (in $R$)

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):

In the cyclic process shown in the figure,the work done by the gas in one cycle is (in $,{P_1}{V_1}$)

What is a cyclic process? Write a note on it.