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posted by  Legolas on 2/24/2008 12:02:08 AM  |  status: Closed  

Chemical Equilibrium

Course Textbook Chapter Problem
General Chemistry N/A N/A N/A
Question Details:
2NO(g) + Cl2(g) <-> 2 NOCl(g)
Kc = 4.6x10^4
Temperature = 298K
In a 1.50L flask there are 4.125 mol of NOCl and 0.1125 mol of Cl2 present at equilibrium
 
What is the partial pressure of NO at equilibrium?
 
What is the total pressure of the system at equilibrium?
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posted by thatsme on 2/24/2008 12:37:54 AM  |  status: Live
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Legolas's comment:
"THANK YOU SOOOO MUCH!!!!"
Response Details:
use formula Kp=Kc(RT)Δngas= (the difference in stoich coefficent products-reactants) to solve for pressure constant
=4.6*10^4(0.082*298)-1
=1882
P=MRT= substituted M for n/v in ideal gas equation
PNOCl= 2.75*0.082*298=67
PCl2=1.83 atm
1882=(PNOCl)2/ (PNO)2(Cl2)
1882=(67)^2/ (PNO)^2(1.83)
PNO= 1.14 atm
total pressure is added up all pressures= 1.14+67+1.83=70 atm
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