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 .

d is the answer i came up with

as we know our atmosphere or air have different levels. every level has other gasses, and every gas has another permeability. when the light comes from lower permeability to higher permeability, it changes its direction. so that means that when the light comes from the moon to the earth, it changes it's direction many more times. it basically means that the shape of the light part of the moon is changed on the earth.

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