Question

Example 50 400 mL of CO gas at 600 mm Hg and 600 mL of He gas at 200 mm Hg are
mixed in a vessel of 1.2 L capacity. Calculate the partial pressure and total pressure of
gaseous mixture. Assume same temperature throughout.​

Answer 1

Answer:

Partial pressures are determined by the mole fraction of the gas in the mixture, thus there are no specific values for gases. For example, if a mixture contains 1 mole of gas A and 2 moles of gas B and the total pressure is 3 atm.

Answer 2

Answer:

Temperature is constant.

So,

For CO₂,

Volume = 400 mL

Pressure = 600 mm Hg

For He,

Volume = 600 mL

Pressure = 200 mm Hg

Total Volume (v) = 1200 mL

Let P' be the partial pressure of CO₂ and P'' of He.

So,

P'v = P₁V₁

P' = P₁V₁/v

= [600*400] / 1200

= 240000/1200

= 200 mm Hg

P''v = P₂V₂

P'' = P₂V₂/v

= [200*600]/1200

= 120000/1200

= 100 mm Hg

Total Pressure (P) = P'+P''

= 100+200 mm Hg

= 300 mm Hg

Hope This Helps.