Asystem undergoes a two-step process. in the first step, the internal energy of the system increases by 218 j when 170 j of work is done on the system. in the second step, the internal energy of the system increases by 107 j when 172 j of work is done on the system.
1. for the overall process, find the heat?
2. what type of process is the overall process? explain.

1) Q total = Q1 +Q2 = 48 J + (-65J) = (-17J)

2) since the total heat exchanged is negative, the overall process is a cooling process

Explanation:

According to the first law of thermodynamics

ΔE = Q - W

where ΔE= change in internal energy , Q = heat and W= work done by the system to the surroundings

in the first step

Q1 = ΔE + W = 218 J  + (-170 J) = 48 J

in the second step

Q2 = ΔE + W = 107 J  + (- 172 J) = -65 J

the total heat is

Q total = Q1 +Q2 = 48 J + (-65J) = (-17J)

since the total heat exchanged is negative, the overall process is a cooling process .

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