Click to Chat

1800-1023-196

+91-120-4616500

CART 0

• 0

MY CART (5)

Use Coupon: CART20 and get 20% off on all online Study Material

ITEM
DETAILS
MRP
DISCOUNT
FINAL PRICE
Total Price: Rs.

There are no items in this cart.
Continue Shopping
`        A container holds 22.4 litre of a gas at 1 atmospheric pressure and at 0°C. The gas consist of a mixture of argon, oxygen, and sulphur dioxide in which :(a) Partial Pressure of SO2 = (Partial Pressure of O2) + (Partial Pressure of Ar).(b) Partial Pressure of O2 = 2 × Partial Pressure of Ar.Calculate the density of the gas mixture under these conditions. `
5 months ago

Rahul
39 Points
```							(a) PSO2=PO2+PAr = 3PAr.       [using (b)]Now from Dalton's law of partial pressure PSO2+PO2+PAr=1=> 3PAr+2PAr+PAr =1=>   PAr =1/6         PO2=1/3        PSO2=1/2Now using PV=nRTWe get no. of moles =PV/RT= 0.9994Now as we know, PAr =mole fraction of Ar *PTotalMole fraction of Ar =1/6 Moles of Ar/ Total no. of moles = 1/6 So, no of moles of Ar = 0.9994/6 = 0.16Similarly, moles of O2 =0.9994/6 = 0.33Moles of SO2 = 0.9994/6 = 0.499Also, moles = Mass/Molecular weightMass of Ar = 6.4Mass of O2 =10.56Mass of SO2= 31.36Total mass =48.32Density = Mass/volume =48.32/22.4 = 2.157 Hope it helpsMe Rahul from Kurukshetra, Haryana
```
5 months ago
Think You Can Provide A Better Answer ?

## Other Related Questions on Physical Chemistry

View all Questions »

### Course Features

• 731 Video Lectures
• Revision Notes
• Previous Year Papers
• Mind Map
• Study Planner
• NCERT Solutions
• Discussion Forum
• Test paper with Video Solution

### Course Features

• 141 Video Lectures
• Revision Notes
• Test paper with Video Solution
• Mind Map
• Study Planner
• NCERT Solutions
• Discussion Forum
• Previous Year Exam Questions