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.

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)

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

c because the news are a source of information of things that happen on the daily and shows evidence about that particular topic

answer: 2×10^-2kg

explanation: density= mass per volume

vol=mass/density

converting to s.i units we have;

3÷1000kg = 0.003

1.5÷100m = 0.15

0.003/0.15 = 0.02kg