Problem: A gas mixture contains 1.26 g N2 and 0.86 g O2 in a 1.56-L container at 18 oC.You want to reference (Pages 216 - 222) Section 5.6 while completing this problem.Calculate the partial pressure of N2.

FREE Expert Solution

We are asked to calculate the partial pressure of O2.


Molar mass O2 = 32.00 g/mol

Molar mass N2 = 28.02 g/mol


Calculate moles each: 

mol O2 = 1.26 g O2 ×1 mol  O232.00 g O2  = 0.039 mol O2 mol N2 = 0.86 g N2 ×1 mol  N228.02 g N2 = 0.031 mol N2

Calculate mole fraction N2 :

XN2 = mol N2mol totalXN2 = mol N2mol totalXN2 = 0.031 mol0.039 mol + 0.031 molXN2 = 0.031 mol0.070 mol

XN2 = 0.443 


Given:

R = 0.08206 L-atm/mol-K

T = 18 oC +273.15 = 291.15 K

V= 1.56 L

n = 0.070 mol


Calculate total pressure: 

PV = nRTP = nRTVP = (0.070 mol)(0.08206  L-atm mol- K)(291.15 K)1.56 L

P = 1.07 atm


94% (42 ratings)
View Complete Written Solution
Problem Details
A gas mixture contains 1.26 g N2 and 0.86 g O2 in a 1.56-L container at 18 oC.

You want to reference (Pages 216 - 222) Section 5.6 while completing this problem.

Calculate the partial pressure of N2.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Partial Pressure concept. You can view video lessons to learn Partial Pressure. Or if you need more Partial Pressure practice, you can also practice Partial Pressure practice problems.