Question

what will be the pressure exerted by a mixture of 3.2g of methane and 4.4g of carbon dioxide contained in a 9dm³ flask at 27°c. ​

Answer 1

Let's apply Ideal gas law: P V = n R T

T = 300°K.

V = 9 dm^3 = 9 * 10⁻³ m³ or  9 L

Molecular mass of Methane: CH4 =16.

               of Carbon Dioxide CO2 = 44.

Total Number of moles of the gases in the mixture:

         n = n1 + n2

            = 3.2/16 + 4.4/44

            = 0.3 mol

R = 8.318 J/°K

P = n R T / V

   = 0.3 mol × 8.314 J/°K/mol × 300°K / 0.009m³ 

P = 0.8314 bar  or  8.314 * 10⁴ Pa   or 0.83 atm

  We can also calculate the partial pressure exerted by Methane and Carbon DIoxide individually. .

     P1 = n1/(n1+n2) * P

     P2 = n2/(n1+n2) *P