i) What will be pressure exerted by a mixture of 3.2 gm of methane and 4.4 g of carbon dioxide
contained in a 9dm3 flask of 270C?
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Answer:
Let's apply ldeal gas law: PV =nRT
T = 300°K.
V = 9 dm³ = 9 × 10^-3 m³ or 9L
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 = nRT/V
= 0.3 molx 8.314 J/K/mol x 300°K /
O.009m³
P = 0.8314 bar or 8.314×10^4Pa or 0.83 atmn
We can also calculate the partial pressure exerted by Methane and
Carbon Dloxide individually..
P1 = n1/(n1+n2) *P
P2 = n2/(n1+n2) *P
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