Question

A gas releases 467 J of heat and expands against an external pressure of 3.6 atm. If

its volume increases by 2.8 L, what is the change in internal energy (AU) of the
system?

Answer 1

The change in internal energy of the system can be determined using the first law of thermodynamics, which states that the change in internal energy is equal to the heat transferred to the system minus the work done by the system. In this case, the change in internal energy is 477.08 J.

Step-by-step explanation:

The change in internal energy (AU) of the system can be determined using the first law of thermodynamics, which states that the change in internal energy is equal to the heat transferred to the system minus the work done by the system:

ΔU = Q - W

In this case, the heat transferred to the system is 467 J and the work done by the system is given by the formula:

W = -PΔV

where P is the external pressure and ΔV is the change in volume. Substituting the given values, we have:

W = -(3.6 atm)(2.8 L) = -10.08 J

Therefore, the change in internal energy of the system is:

ΔU = 467 J - (-10.08 J) = 477.08 J