Calculate the work done when 1.000 mole of an ideal gas expands reversibly from 1.0 l to 10 l at 298.0 k. then, calculate the amount of work done when 1.000 mole of an ideal gas at 298.0 k expands irreversibly against a constant external pressure of 1.00 atm. compare the two values and comment. the question continues at the bottom.
wrev=-nrtln(vf/vi)
-(1.000 mol)(0.08205 l*atm/mol*k)(298k)ln(10l/1l).
=-(56.3 l*atm) (101.325 j/ l*atm)
=-5705j
my question is where do the values 56.3 l*atm and 101.325 j/ l*atm come from, what are they derived from? when i multiplied -(1.000 mol)(0.08205 l*atm/mol*k)(298k)ln(10l/1l) i get -129.63 l*atm/k. this was a completed example i was given in class and i couldn't break it down.
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Calculate the work done when 1.000 mole of an ideal gas expands reversibly from 1.0 l to 10 l at 298...
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