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?
dE = q+w
q = -202.90+(+315.7)
112.8
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.