Question

What will be the pressure exerted by a mixture of 5.6 g of N 2 and 6.4 g of CH 4
contained in a 12 dm 3 flask at 37 °C?

Answer 1

Answer:

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

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