The work done to contract a gas in a cylinder is $462 \, J$. $128 \, J$ of energy is evolved in the process. What will be the internal energy change in the process? (in $J$)

If $Q$ is the heat liberated from the system and $W$ is the work done on the system,then the first law of thermodynamics can be written as:

In an adiabatic process,no transfer of heat takes place between the system and surroundings. Choose the correct option for the free expansion of an ideal gas under adiabatic conditions from the following:

Which of the following set of properties is correct when one mole of a gas is heated keeping volume constant by increasing temperature and supplying $500 \ J$ of heat?

Which one of the following is applicable for an adiabatic expansion of an ideal gas?

Calculate the change in internal energy of the system if $20 \ kJ$ work is done on the system and it releases $10 \ kJ$ heat in a particular reaction. (in $kJ$)