Question

During the isobaric expansion from A to B represented below, 3,100 J of heat are added to the gas. What is the change in its internal energy?

(a) 2,900 J
(b) 3,100 J
(c) 6,200 J
(d) 0 J

Answer 1

The change in internal energy (ΔU) of the gas is equal to the amount of heat added to the gas, which in this case is 3,100 J.

Step-by-step explanation:

The change in internal energy (ΔU) of a gas can be calculated using the first law of thermodynamics, which states that the change in internal energy is equal to the heat added to the gas minus the work done by the gas. The change in internal energy (ΔU) of the gas is equal to the amount of heat added to the gas, which in this case is 3,100 J.

In this case, the gas is expanding isobarically, which means its pressure remains constant. Since heat is added to the gas, the change in internal energy (ΔU) will be equal to the amount of heat added, which is 3,100 J.

Therefore, the correct answer is (b) 3,100 J.