1.

Two moles of ammonia were found to occupy a volume of 5 L at 27^(@)C. Calculate the pressure using van der Waals equation (a="4.17 bar L"^(2)"mol"^(-2), b="0.0371 L mol"^(-1)).

Answer»

Solution :n= 2
V = 5 LITRES
`T = 273 + 27 = 300 K`
`a = 41.7 "atm lit"^(2) "mole"^(-2)`
`b = 0.0371 "lit mole"^(-1)`
`R = 0.082 "lit atm deg"^(-1) "mole"^(-1)`
Applying van der Waals equation for n moles
`(p + (a n^(2))/(V^(2))) (V-n b) = nRT`
`(p+(4.17 xx 2^(2))/(5^(2))) (5-2 xx 0.0371) = 2 xx 0.082 xx 300`
p = 9.33 atm.


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