First Law of Thermodynamics

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 $\frac{Q}{5}$  when heat Q is supplied to it. The molar heat capacity of the gas during this transformation is  The value of x is $\frac{xR}{8}.$ ………

[R = universal gas constant]

Three different processes that can occur in an ideal monoatomic gas are shown in the P vs V diagram. The paths are labeled as A → B, A → C and A → D. The change in internal energies during these process are taken as EAB, EAC and EAD and the work done by WAB, WAC and WAD. The correct relation between these parameters are:

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:

Match the thermodynamics processes taking place in a system with the correct conditions. In the table: $\mathrm{\Delta }\mathrm{Q}$ is the heat supplied, $\mathrm{\Delta }\mathrm{W}$ is the work done and $\mathrm{\Delta }\mathrm{U}$  is change in internal energy of the system. Match the following: