Calculate the work done when 1.000 mole of a perfect gas expands reversibly from 1.0 L to 10 L at 298.0 K. Then, calculate the amount of work done when the gas expands irreversibly against a constant external pressure of 1.00 atm. Compare the two values and comment.

See explanation

Explanation:

For work done at constant temperature;

w = -nRTln(V2/V1)

V1 = 1.0 L

V2 = 10 L

w = -(1 * 8.314 * 298) ln(10/1)

w = -5704.8 J

When the gas expands irreversibly against a constant external pressure;

w = -(PΔV)

w = -(1.00 (10 - 1))

w = - 9 J

During expansion of a gas in which the initial and final limits of volume are given, the constant pressure process produces more work than the isothermal process as we have seen above.

water at room temperature is flowing through a pipe with pressure taps located 10 ft apart along one section of the pipe, which are connected to a mercury (s=13.6) manometer.