Question

What is the total internal energy change (∆E), in J, of a system that releases 202.90 J of heat and absorbs 315.7 J of work from the surroundings?

Answer 1

dE = q+w

q = -202.90+(+315.7)

Answer 2

112.8

Answer 3

[AI-generated answer — Explain Bot]

To determine the total internal energy change (∆E) of a system, you can use the First Law of Thermodynamics, which states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system on the surroundings. Mathematically, it can be expressed as:

∆E = Q - W

where ∆E represents 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, we are given that the system releases 202.90 J of heat (Q = -202.90 J) and absorbs 315.7 J of work (W = 315.7 J).

To find the total internal energy change (∆E), we substitute the given values into the equation:

∆E = -202.90 J - 315.7 J

By performing the calculation, we get:

∆E = -518.60 J

Therefore, the total internal energy change (∆E) of the system is -518.60 J. Note that the negative sign indicates that the internal energy of the system has decreased.