Considering air as a 4:1 mixture of nitrogen and oxygen, what is the density of air at 25 °C and
1 atm?
1 atm?
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The volume of 1 mole of a gas at 25°C is
22.4L x 298K/273K = 24.45L
The densities of the elements at 25°C are
O2: 32.0g/24.45L = 1.309g/L
N2: 28.0g/24.45L = 1.145g/L
A weighted average of the two gases is
(4 x 1.145 + 1 x 1.309) / 5 = 1.178g/L which you probably ought to round to 3 digit like 22.4L or the molar masses = 1.18g/L
22.4L x 298K/273K = 24.45L
The densities of the elements at 25°C are
O2: 32.0g/24.45L = 1.309g/L
N2: 28.0g/24.45L = 1.145g/L
A weighted average of the two gases is
(4 x 1.145 + 1 x 1.309) / 5 = 1.178g/L which you probably ought to round to 3 digit like 22.4L or the molar masses = 1.18g/L