Calculate q, and determine whether heat is absorbed or released when a system does work on the surroundings equal to  69.0 J  and  Δ U = −219.0 J.

An 80.0 g sample of a gas was heated from 25 °C to 225 °C. During this process, 346 J of work was done by the system and its internal energy increased by 9095 J. What is the specific heat of the gas?

A gas is compressed from 2.31 L down to 1.12 L at a pressure of 1.13 atm. If 51 J of heat is given off in the process, what is the change in the internal energy ΔU of the gas?

What is the change in internal energy for a system if the system absorbs 322 kJ of heat and has 750.0 kJ of work done on the system?

As a system increases in volume, it absorbs 55.0 J of energy in the form of heat from the surroundings. The piston is working against a pressure of 0.540 atm. The final volume of the system is 58.2 L. What was the initial volume of the system if the internal energy of the system decreased by 103.4 J?

Calculate ΔU of a gas for a process in which the gas absorbs 41 J of heat and does 8 J of work by expanding.

I don’t get this

Calculate the internal energy (in Joules) of an endothermic system that absorbs 370.8 J and expands from 1.00 to 10.32 L against a pressure of 4.64 atm.