Question

A mixture of xenon and argon gases, in a 9.76 l flask at 76 °c, contains 42.2 grams of xenon and 13.4 grams of argon. What is the partial pressure of argon in the flask? What is the total pressure in the flask?

Answer 1

To calculate the partial pressure of argon in the flask, we need to calculate the mole fraction of argon and multiply it by the total pressure. The total pressure in the flask is given as 1.00 atm.

Step-by-step explanation:

To find the partial pressure of argon in the flask, we need to calculate the mole fraction of argon and then multiply it by the total pressure.

First, calculate the number of moles of xenon and argon:

Moles of Xenon (Xe) = 42.2 g / molar mass of Xenon

Moles of Argon (Ar) = 13.4 g / molar mass of Argon

Next, calculate the mole fraction of argon:

Mole fraction of Ar = Moles of Ar / (Moles of Xe + Moles of Ar)

Finally, calculate the partial pressure of argon by multiplying the mole fraction by the total pressure:

Partial pressure of Ar = Mole fraction of Ar * Total pressure

To find the total pressure in the flask, simply use the given value of 1.00 atm.