Gaseous StateHard
Question
What is the total pressure exerted by the mixture of 7.0 g of N2, 2g of hydrogen and 8.0 g of sulphur dioxide gases in a vessel of 6 L capacity that has been kept in a reservoir at 27oC?
Options
A.2.5 bar
B.4.5 bar
C.10 atm
D.5.7 bar
Solution
No. of moles of N2 = 
No. of moles of H2 = 1 Mole Total moles =
+ 1 + 
No. of moles of SO2 =
moles = 
(2 + 8 + 1) = 
P =
= 5.64 ≈ 5.7 atm.
No. of moles of H2 = 1 Mole Total moles =
+ 1 + No. of moles of SO2 =
moles = (2 + 8 + 1) = P =
= 5.64 ≈ 5.7 atm. Create a free account to view solution
View Solution FreeMore Gaseous State Questions
One litre of a gaseous mixture of two gases effuses in 311 seconds while 2 litres of oxygen takes 20 minutes. The vapour...NH3 gas is liquefied more easily than N2. Hence:...Helium atom is two times heavier than a hydrogen molecule. At 298 K, the average kinetic energy of a helium atom is...Calculate the compressibility factor for CO2, if one mole of it occupies 0.4 litre at 300 K and 40 atm. Comment on the r...What volume will be occupied by a sample of gas at 40oC and 720 mm μg if its volume at 20oC and 750 mm μg was ...