One mole of an ideal gas is expanded from a volume of 1.00 liter to a volume of 6.43 liters against a constant external pressure of 1.00 atm. how much work (in joules) is performed on the surroundings? ignore significant figures for this problem. (t = 300 k; 1 l·atm = 101.3 j)

Question

Eliana Robertson

Chemistry

10 September, 00:49

One mole of an ideal gas is expanded from a volume of 1.00 liter to a volume of 6.43 liters against a constant external pressure of 1.00 atm. how much work (in joules) is performed on the surroundings? ignore significant figures for this problem. (t = 300 k; 1 l·atm = 101.3 j)

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Aldo Haynes · Answer 1

We actually don't need the value for temperature. There is a direct formula relating work, pressure and volume. The relationship is:

W = Pexternal (ΔV)

Substituting the values and incorporating the conversion ratio,

W = (1 atm) (6.43 L - 1 L) (101.3 J/1 L·atm)

W = 651.36 J