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Pie
1 month ago
8

3. A sample of argon of mass 6.56 g occupies 18.5 dm? at 305 K. (a) Calculate the work done when the gas expands isothermally ag

ainst a constant external pressure of 7.7 kPa until its volume has increased by 2.5 dm'. (b) Calculate the work that would be done if the same expansion occurred reversibly.
Physics
1 answer:
serg [3.5K]1 month ago
4 0

Response:

(a) W=-19.25J

(b) W=-52.8J

Clarification:

Greetings.

(a) In this case, since the starting volume is 18.5 dm³ and the ending volume is 21 dm³ (18.5 +2.5), we can calculate the work at constant pressure as shown below:

W=-P\Delta V=-7.7kPa*\frac{1000Pa}{1kPa} (21dm^3-18.5dm^3)*\frac{1m^3}{1000dm^3}\\ \\W=-19.25J

This value is negative as it expands against the given pressure.

(b) Furthermore, if the process is conducted reversibly, the pressure might change, hence, we need to calculate the work using:

W=nRTln(\frac{V_1}{V_2} )

The moles are calculated based on the provided mass of argon:

n=6.56g*\frac{1mol}{39.95g}=0.164mol

Consequently, the work amounts to:

W=0.164mol*8.314\frac{J}{mol*K} *305Kln(\frac{18.5dm^3}{21dm^3} )\\\\W=-52.8J

Best regards.

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