Home
Class 11
CHEMISTRY
A gaseous mixture contains three gases A...

A gaseous mixture contains three gases A,B and C with a total number of moles of 10 and total pressure of 10 atm. The partial pressure of A and B are 3 atm and 1 atm respectively. If C has molecular weight of 2 g/mol. then, the weight of C present in the mixture will be :

A

8

B

12

C

3

D

6

Text Solution

Verified by Experts

The correct Answer is:
B
`P = 10 atm, n_(A) + n_(B) + n_(C) = 10`
`p_(A) = 3.0 atm, p_(B) = 1.00 atm`
`p_(A) = underset(n_(A) + n_(B) + n_(C))overset(n_(A))rarr P`
`3.00 = (n_(A))/(10) 10 rArr n_(A) = 3.00`
Similarly, `n_(B) = 1.00`
`n_(C) = (n_(A) + n_(B) + n_(C)) - (n_(A) + n_(B))`
`= 10-(3 + 1) = 6`
Mass of gas `C = n_(C) xx` Mol. mass of C
`= 6 xx 2 = 12`
`n = (2.8)/(28) = 0.1`
Promotional Banner

Similar Questions

Explore conceptually related problems

A gaseous mixture contains three gaseous A,B and C with a total number of moles of 10 and total pressure of 10 atm . The partial pressure of A and B are 3 atm and 1 atm respectively and if C has molecular weight of 2 g //mol . Then, the weight of C present in the mixture will be :

56 g of nitrogen and 96 g of oxygen are mixed isothermaly and at a total pressure of 10 atm. The partial pressures of oxygen and nitrogen (in atm) are respectively :

A gaseous mixture contains 56 g of N_2 , 44 g CO_2 and 16 g of CH_4 The total pressure of the mixture is 720 mm Hg. The partial pressure of CH_4 is

A methane +H_(2) mixture contains 10g methane and 5g Hydrogen. If the pressure of the mixture is 30 atm. What is the partial pressure of H_(2) in mixture :-

Equal mass of H_(2) , He and CH_(4) are mixed in empty container at 300 K, when total pressure is 2.6 atm The partial pressure of H_(2) in the mixture is

The pressure of a mixture of equal weight of two gases of mol wt. 4 and 40, is 1.1 atm. The partial pressure of the lighter gas in this mixture is

In a ten litre vessel, the total pressure of a gaseous mixture containing H_(2), N_(2) and CO_(2) is 9.8atm. The partial pressures of H_(2) and N_(2) are 3.7 and 4.2 atm respectively. Then the partial pressure of CO_(2) is

For the reaction C(s)+CO_(2)(g) hArr 2CO(g) , the partial pressure of CO_(2) and CO is 5.0atm amd 10 atm, respectively, at equilibrium. The K_(p) of the reaction is

An ideal mixture of liquids A and B with 2 moles of A and 2 moles of B has a total vapour pressure of 1 atm at a certain temperature. Another mixture with 1 mole of A and 3 moles of B has a vapour pressure greater than 1 atm. But if 4 moles of C are added to second mixture, the vapour pressure comes down to 1 atm. Vapour pressure of C, P_(C)^(@)=0.8 atm. Calculate the vapour pressure of pure A and B :

In a mixture of N_2 and CO_2 gases, the partial pressure of CO_(2) is 1.25 atm. The total pressure of the mixture is 5 atm. The mole fraction of N_(2) in the mixture is