In a thermodynamic process, pressure of fixed mass of a gas is changed in such a manner that the gas releases 20 J of heat and 8 J of work is done on the gas. If initial internal energy of the gas was 40 J, what will be final internal energy?

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

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

1 mole of rigid diatomic gas performs a work of $\frac{Q}{5}$ <!-- [if gte mso 9]><xml> </xml><![endif]--> when heat Q is supplied to it. The molar heat capacity of the gas during this transformation is <!-- [if gte mso 9]><xml> </xml><![endif]--> The value of x is $\frac{xR}{8}.$ ………

[R = universal gas constant]

A sample of an ideal gas is taken through the cyclic process ABCA as shown in figure. It absorbs, 40 J of heat during the part AB, no heat during BC and rejects 60 J of heat during CA. A work of 50 J is done on the during the part BC. The internal energy of the gas at A is 1560 J. The work done by the gas during the part CA is: