A gas in a system has constant pressure. The surroundings around the system lose 62 J of heat and does 474 J of work onto the system. What is the internal energy of the system?*5 points412 J536 J29,388 J7.65 J

The internal energy of a system can be calculated using the first law of thermodynamics, which states that the change in internal energy (ΔU) of a system is equal to the heat added to the system (Q) minus the work done by the system (W). In mathematical terms, this is expressed as:

ΔU = Q - W

In this case, the surroundings lose 62 J of heat, which means that the system gains 62 J of heat (Q = +62 J). The surroundings also do 474 J of work onto the system, which means that the system has work done on it (W = -474 J).

Substituting these values into the equation gives:

ΔU = 62 J - (-474 J) = 62 J + 474 J = 536 J

Therefore, the internal energy of the system is 536 J.

The internal energy of a system can be calculated using the first law of thermodynamics, which states that the change in internal energy (∆U) of a system is equal to the heat added to the system (Q) minus the work done by the system (W). In mathematical terms, this is expressed as ∆U = Q - W.

In this case, the surroundings lose 62 J of heat, which means that the system gains 62 J of heat (Q = +62 J). The surroundings also do 474 J of work onto the system, which means that the system has work done on it (W = -474 J).

Substituting these values into the equation gives:

∆U = Q - W ∆U = 62 J - (-474 J) ∆U = 62 J + 474 J ∆U = 536 J

So, the internal energy of the system is 536 J.