Question

Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 24.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 24.0L. Now calculate the work done if this process is carried out in two steps. 1. First, let the gas expand against a constant external pressure of 1.50 atm to a volume of 16.0L. 2. From the end point of step 1, let the gas expand to 24.0 L against a constant external pressure of 1.00 atm.

Answer 1

A.

work = P_external * Volume change

-1 atm * (24-1) = -23 atm-L

in general 1atm-L =101.324999971J

so -23 atm-L = -23 X 101.324999971J = -2330.5 J

work (w) = -2330.5 J

B.

calculate each step individually then sum the answers

for step 1)

-1 * 1,50 * (16-1) = -22.5 atm-L

for step 2)

-1* (24-16) = -8 atm-L

thus total work = -30.5 atm-L

on converting to joules

1 atm-L = 101.325 J

-30. atm-L = -3090.41 J

work done = -3090.41 J

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