Question

ne mole of an ideal gas is expanded from a volume of 1.00 liter to a volume of 8.41 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.

Answer 1

Complete question

One mole of an ideal gas is expanded from a volume of 1.00 liter to a volume of 8.41 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)

Step-by-step explanation:

Given that,

Number of mole

n = 1 mole

Initial volume

Vi = 1 litre

Final Volume

Vf = 8.41 litre

Constant Pressure

P = 1 atm

Work done in Joule?

Work done under constant pressure is given as

W = P∆V

W = P(Vf—Vi)

W = 1 atm × (8.41—1) litre

W = 1 atm × 7.41 litre

W = 7.41 Litre•atm

Given that,

1 Litre•atm = 101.3J

Then,

W = 7.41 Litre•atm × 101.3J/Litre•atm

W = 750.633 J

W ≈ 751J

Then the work done on the surrounding is approximately

751 joules