A1.05-l bulb and a 1.52-l bulb are connected by a stopcock and filled, respectively, with argon at 0.72 atm and helium at 1.08 atm at the same temperature. calculate the total pressure, the partial pressures of each gas, and the mole fraction of each gas after the stopcock has been opened. assume ideal-gas behavior. (answer in 3 significant figures)

Explanation:

We have given that A 1.05-L bulb and a 1.52-L bulb are connected by a stopcock and filled with argon at 0.72 atm and helium at 1.08 atm  respectively, at the same temperature.

Let P₁(p) be the partial pressure of gas in bulb A then

Similarly, Let be the partial pressure of gas in bulb B then

Total pressure= 0.294 + 0.638 = 0.932atm

If n₁ and n₂ be their moles in the respective bulbs

P₁V₁ = n₁ R t

P₂ V₂ = n₂ R t

Now,

Mole fraction of argon = 0.316

Mole fraction of helium = 0.685

hello, i am papaguy.

i have found an answer to your question but use it as information.

information: because weak acids/bases have low concentration of hydrogen ions, the addition of water has a large impact on the ph. 2. a difference in 1 unit is a 10x difference in concentration for example; a liquid with ph of 3 is 10x more acidic than a liquid with a ph of 4. therefore, a liquid with a ph of 3 is stronger.

best of luck!