What is the partial pressure of each gas inside container? the mole fraction of each cmpd in artficial atms?

Question

an artificial atmosphere for the planet mars consists of 80% carbon dioxide gas (CO2) 15% methane gas (CH4) and 5% nitrogen gas (N2). 10.0g of this gas mixture is placed in a 100L container at temperature of 4 degre Celcius .

Answer 1

In 10.0 g of mixture there are 8.0 g CO2 ( =8.0 / 44 = 0.182 mole ), 1.5 g CH4 ( = 1.5 / 16 = 0.937 mole ) and 0.50 g N2 ( = 0.50 /28 = 0.0178 mole )
The partial pressure is defined as the individual pressure one component exerts treating it as if it were all by itself in the continer.

p = n R T / V
T = 4 + 273 = 277 K V= 100 L R = 0.08206

p(CO2) = 0.182 (0.08206) (277) /100 = 0.0414 atm

p(CH4) = 0.937 ( 0.08206) (277) / 100 = 0.213 atm

p(N2) =0.0178 (0.08206) (277) / 100 = 0.00404 atm

Answer 2

firstly find the mass,m of each gas e.g for CO2:
80/100 x 10 = 8g
Then use the gas equation to find partial pressure
PV = nRT....
n= no of moles = mass of gas/ molar mass
T = temp in Kelvin = 4 +273 = 277K
Volume = 100L = 0.1m^3
R = constant = 8.314
so for CO2
P = (8 x 8.314 x 277)/(44 x 0.1)
P= 4187.23 N/m^2 .......... this is the partial pressure of CO2
Now do the same for all the other gases