Answer:
(a) W₁ = 3293.06 J = 3.293 KJ
(b) W₂ = 0 J
(c) W₃ = - 506.625 J = - 0.506 KJ
(d) W₄ = 0 J
(e) W = 2786.435 J = 2.786 KJ
Explanation:
The complete question has following parts:
(a) First gas expands from a volume of 1 L to 6 L at a constant pressure of 6.5 atm
(b) Second, the gas is cooled at constant volume until the pressure falls to 1 atm
(c) Third, the gas is compressed at a constant pressure of 1 atm from a volume of 6 L to 1 L.
(d) Finally the gas is heated until its pressure from 1 atm to 6.5 atm at constant volume
(e) what is the net work?
<u>ANSWERS:</u>
(a)
The work done by a gas at constant pressure is given as follows:
W = PΔV
where,
W = Work done by the gas
P = Constant Pressure of the Gas
ΔV = Change in Volume of The gas
Therefore, for the first step:
P = P₁ = (6.5 atm)(1.01325 x 10⁵ Pa/1 atm) = 6.58613 x 10⁵ Pa
ΔV = ΔV₁ = 6 L - 1 L = (5 L)(0.001 m³/1 L) = 5 x 10⁻³ m³
W = W₁
Therefore,
W₁ = (6.58613 x 10⁵ Pa)(5 x 10⁻³ m³)
<u>W₁ = 3293.06 J = 3.293 KJ</u>
(b)
The work done at a constant volume by a gas is always zero due to no change in volume:
W₂ = P₂ΔV₂
W₂ = P₂(0)
<u>W₂ = 0 J</u>
<u></u>
(c)
For the third step:
P = P₃ = (1 atm) = 1.01325 x 10⁵ Pa
ΔV = ΔV₃ = 1 L - 6 L = (- 5 L)(0.001 m³/1 L) = - 5 x 10⁻³ m³
W = W₃
Therefore,
W₃ = (1.01325 x 10⁵ Pa)(-5 x 10⁻³ m³)
<u>W₃ = - 506.625 J = - 0.506 KJ</u>
(d)
The work done at a constant volume by a gas is always zero due to no change in volume:
W₄ = P₄ΔV₄
W₄ = P₄(0)
<u>W₄ = 0 J</u>
<u></u>
(e)
Hence, the net work is given as follows:
W = W₁ + W₂ + W₃ + W₄
W = 3293.06 J + 0 J + (- 506.625 J) + 0 J
<u>W = 2786.435 J = 2.786 KJ</u>
