Argon Nitrogen

A sample of air contains 74.25% nitrogen, 24.90% oxygen, 0.05% carbon dioxide, and 0.80% argon, by volume. How?

A sample of air contains 74.25% nitrogen, 24.90% oxygen, 0.05% carbon dioxide, and 0.80% argon, by volume. How many molecules of each gas are present in 1.00 L of the sample at 25°C and 1.00 atm?

The composition of each gas in the volume of 1 L are obtain by multiply the percentage and the volume

Volume gas
= % x Volume of sample

from the formula above we get each gas volumes:

N2 = 0.7425 L
O2 = 0.2490 L
CO2 = 5.10exp-4 L
Ar = 8.10exp-3 L

next use the formula of ideal gas to find the mole of each gas

PV = nRT solve for the “n”

n = PV/RT

n is the mole, P is pressure, V is volume T temperature in Kelvin and R is the gas constant 0.08206

moles of N2 = (1 x 0.7425) / (0.08206 x 298) = 0.030 mol

and with the same way we get the moles of

O2 = 0.010 mol
CO2 = 2.05.10exp-5 mol
Ar = 3.271.10exp-4 mol

The number of molecules in each gas are obtain by:

Number of molecules = N x mole

N is the avogadro number that is 6.022.10exp23

thus

N2 = 1.81.10exp23 molecules
O2 =6.022.10exp21molecules
CO2 =1.235.10exp19 molecules
Ar = 1.98.10exp20 molecules

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