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 ?
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, nCH4 = 3.2/ 16 = 0.2 mol
& amount of CO2 nCO2 = 4.4/ 44 = 0.1 mol
Also we know ,
Pv = (nCH4 + nCO2) RT
OR P X 9 = (0.2 +0.1) x 0.0821 x 300
Or p = 0.3 x 0.0821 x 300 / 9 = 0.821 atm
Hence, the total pressure exerted by the mixture is 0.821 atm
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