A1.00 l flask is filled with 1.30 g of argon at 25 ∘c. a sample of ethane vapor is added to the same flask until the total pressure is 1.300 atm . part a what is the partial pressure of argon, par, in the flask? express your answer to three significant figures and include the appropriate units. view available hint(s) parp a r p_ar = nothing nothing part b what is the partial pressure of ethane, pethane, in the flask?

Answer :

Part A : The partial pressure of argon is, 0.795 atm

Part B : The partial pressure of ethane is, 0.505 atm

Explanation :

Part A :

First we have to calculate the moles of argon.

Molar mass of argon = 39.95 g/mole

Now we have to calculate the partial pressure of argon.

Using ideal gas equation :

PV = nRT

where,

P = Pressure of argon = ?

V = Volume of argon = 1.00 L

n = number of moles of argon = 0.0325 mole

R = Gas constant =

T = Temperature of argon =

Putting values in above equation, we get:

The partial pressure of argon is, 0.795 atm

Part B :

Now we have to calculate the partial pressure of ethane.

As we know that,

Total pressure = Partial pressure of argon + Partial pressure of ethane

1.300 atm = 0.795 atm + Partial pressure of ethane

Partial pressure of ethane = 1.300 - 0.795

Partial pressure of ethane = 0.505 atm

The partial pressure of ethane is, 0.505 atm

b

explanation:

bc its just b