Question

In a process of an ideal gas, the pressure is halved while the volume is kept constant. During this process, 750 J of heat flows out of gas. What is the change in the internal energy of the gas in this process?

(a) -750 J
(b) 750 J
(c) 1500 J
(d) -1500 J

Answer 1

The change in internal energy of the ideal gas when pressure is halved and volume remains constant with 750 J of heat lost is -750 J. The correct answer is option A.

Step-by-step explanation:

When an ideal gas undergoes a process where the pressure is halved while the volume remains constant, and 750 J of heat flows out of the gas, the first law of thermodynamics can be used to determine the change in internal energy of the gas.

The first law of thermodynamics is given by ΔU = Q - W, where ΔU is the change in internal energy, Q is the heat added to the system, and W is the work done by the system. In this case, since no work is done (the volume is constant), the change in internal energy is simply the heat lost by the system, which is -750 J.