Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
Related questions
Question
Expert Solution
Step 1
The partial pressure of an individual gas is equal to the total pressure multiplied by the mole fraction of that gas.
mole fraction is the number of moles of one particular gas divided by the total moles of gas in the mixture.
So, using this concept, we can solve the problem.
Step 2
From the molecular level representation, total number of molecules is 6+5+3 = 14.
So, the number of moles is 14/Na and out of which 3/Na moles are diatomic gas.
So, the mole fraction of diatomic gas is
Xi = nA/(nA+nB+nC)
Xi = 3/14 = 0.214
Now we can find the total pressure as,
Pi = Ptotal × Xi
==> Ptotal = Pi/Xi
= 0.450/0.214
= 2.10 atm
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