A.
The work has a negative value.
Since the gas in the chamber expands, it increases in volume and does positive work on the piston since the change in volume is positive.
Work, W = pΔV. Since the gas expands, ΔV > 0. So, W > 0. Thus Work done by the gas is positive.
Since in ΔU = Q + W, W here is work done by the surroundings, W is negative since it is the opposite of the work done on the surroundings by the gas..
So, the work has a negative value.
B.
The heat added to the gas chamber is 17 J
From the first law of thermodynamics, ΔU = Q + W where ΔU = internal energy change = U₂ - U₁ where U₁ = initial energy = 8 J and U₂ = final energy = 30 J, Q = heat added to the gas chamber and W = work on piston = - 5 J
ΔU = Q + W
U₂ - U₁ = Q + W
30 J - 8 J = Q + (-5 J)
22 J = Q - 5 J
Q = 22 J + 5 J
Q = 27 J
The heat added to the gas chamber is 27 J.
Learn more about first law of thermodynamics here:
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