Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 10.0 atm.?

Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 10.0 atm.

Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm exerted by the surroundings to a final volume of 15.0 L.

Now calculate the work done if this process is carried out in two steps: Step 1: First let the gas expand against a constant external pressure of 5.00 atm to a volume of 3.00 L. Step 2: Now let the gas expand to 15.0 L against a constant external pressure of 1.00

Question

Baylee Swanson

Chemistry

10 April, 01:40

Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 10.0 atm.?

Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 10.0 atm.

Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm exerted by the surroundings to a final volume of 15.0 L.

Now calculate the work done if this process is carried out in two steps: Step 1: First let the gas expand against a constant external pressure of 5.00 atm to a volume of 3.00 L. Step 2: Now let the gas expand to 15.0 L against a constant external pressure of 1.00

+1

Answers (1)

Know the Answer?

Valentin Rodriguez · Answer 1

Work = - Pressure external*Volume change

-1 atm * (20 - 1) = - 19 atm-L.

1 atm-L = 101.324999971 J

So - 19 * 101.32 = - 1925 J

B.

Calculate each step individually then sum the answers.

For step 1)

-5 * (4-1) = - 15 atm-L

step 2)

-1 * (20-4) = - 16 atm-L

Thus total work = - 31 atm-L

convert to joules,

-3141 J