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Question
Find the isothermal irrevesible work done when 2 moles of hydrogen expand from 15 to 50 litres against a constant pressure of 1 atm at 25oC.
Find the isothermal irrevesible work done when 2 moles of hydrogen expand from 15 to 50 litres against a constant pressure of 1 atm at 25oC.
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Solution
The correct option is A -848.2 cal
The formula of work done (W) for an Isothermal Irreversible expansion is
W=−P(V2−V1)
Where V1 is the initial volume of the gas =15L
V2 is the final volume of the gas =50L
W=−1 atm×(50−15)L=−35 L atm
W=−35×101.3 J=−3545.5 J ∵(1 L−atm=101.3 J)
W=−3545.54.18 ∵(1 cal=4.18 J)=−848.2 cal
The formula of work done (W) for an Isothermal Irreversible expansion is
W=−P(V2−V1)
Where V1 is the initial volume of the gas =15L
V2 is the final volume of the gas =50L
W=−1 atm×(50−15)L=−35 L atm
W=−35×101.3 J=−3545.5 J ∵(1 L−atm=101.3 J)
W=−3545.54.18 ∵(1 cal=4.18 J)=−848.2 cal
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