Question

10.
3.2 g of oxygen (At wt.=16) and 0.2 g of
hydrogen (At wt. =1) are placed in a 1.12 L
flask at 0°C. The total pressure of the gas
mixture will be :
(1) 1 atm
(2) 4 atm
(3) 3 atm
(4) 2 atm​

Answer 1

Answer:

According to Dalton law of partial pressure Ptotal = P1 + P2 +.............+ Pn

Hence Ptotal = P oxygen + Phydrogen

P = n RT/ V {using ideal gas equation where symbols have their usual meanings }

number of moles of oxygen = 3.2/ 16

number of moles of hydrogen = 0.2/1 { n is no of moles = given mass/ molar mass }

On substituting values in the ideal gas equation, we get.

= 4.00 atm

= 4.00 atm

Hence P total = 4.00 + 4.00 atm = 8.00 atm