Question

The total mass of the atmosphere is about 5.00 x 1018 kg. How many moles each of air, O2, and CO2 are present in the atmosphere? Note that it is important to work in units of moles rather than in units of mass. By the ideal gas law, PV=nRT. P is pressure, V is volume, n is the number of moles, T is temperature (K), and R is the gas constant. At a given temperature and pressure, the volume is proportional to the number of moles, not to the mass.

Answer 1

Answer: The moles of oxygen and carbon dioxide in air is
`3.63* 10^(19)mol` and
`7.18* 10^(16)mol` respectively

Step-by-step explanation:

To calculate the number of moles, we use the equation:

`\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}`

Given mass of atmosphere =
`5.00* 10^(18)kg=5.00* 10^(21)g`

Average molar mass of atmosphere = 28.96 g/mol

Putting values in above equation, we get:

`\text{Moles of atmosphere}=(5.00* 10^(21)g)/(28.96g/mol)=1.73* 10^(20)mol`

We know that:

Percent of oxygen in air = 21 %

Percent of carbon dioxide in air = 0.0415 %

Moles of oxygen in air =
`(21)/(100)* 1.73* 10^(20)=3.63* 10^(19)mol`

Moles of carbon dioxide in air =
`(0.0415)/(100)* 1.73* 10^(20)=7.18* 10^(16)mol`

Hence, the moles of oxygen and carbon dioxide in air is
`3.63* 10^(19)mol` and
`7.18* 10^(16)mol` respectively