Question

What will be the pressure exerted by a mixture of 3.2 g of methane and 4.4 g of carbon dioxide contained in a 9 dm3 flask at 27 °C ? 

Answer 1

Given,

Mass of carbon dioxide = 4.4 g

Molar mass of carbon dioxide= 44g/mol

Mass of methane  = 3.2g

Molar mass of methane = 16g/mol

Now amount of methane, n_CH4 = 3.2/ 16 = 0.2 mol

& amount of CO₂  n_CO2  = 4.4/ 44 = 0.1 mol

Also we know ,

Pv = (n_CH4 + n_CO2) RT

OR P X 9 = (0.2 +0.1) x 0.0821 x 300

Or  p = 0.3 x 0.0821 x 300 / 9 = 0.82 atm

Hence, the total pressure exerted by the mixture is 0.82 atm

Answer 2

It is known that, 

For methane (CH₄), 

For carbon dioxide (CO₂),