We know that the reverse of the reaction: H2O(g) ↔ H2(g) + 1⁄2O2(g) is rather explosive, yet there is still a finite equilibrium constant of 8.581×10-41 at 298 K. It’s hard to imagine how an equilibrium could exist! How could there be any hydrogen or oxygen gas left over the bang? a. To understand what is going on, first fill out the remaining entries of the table of mole fractions below like in the example from question 1. Let’s assume the pressure is maintained at a constant 1 bar, as such we don’t need to worry about partial pressures etc. b. Using the data above please write the expression for ?? = [(XH2) (Xo2 )^1/2 ] / XH2o using
We know that the reverse of the reaction: H2O(g) ↔ H2(g) + 1⁄2O2(g) is rather explosive, yet there is still a finite equilibrium constant of 8.581×10-41 at 298 K. It’s hard to imagine how an equilibrium could exist! How could there be any hydrogen or oxygen gas left over the bang? a. To understand what is going on, first fill out the remaining entries of the table of mole fractions below like in the example from question 1. Let’s assume the pressure is maintained at a constant 1 bar, as such we don’t need to worry about partial pressures etc. b. Using the data above please write the expression for ?? = [(XH2) (Xo2 )^1/2 ] / XH2o using
Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter7: Reaction Rates And Chemical Equilibrium
Section: Chapter Questions
Problem 7.25P
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We know that the reverse of the reaction:
H2O(g) ↔ H2(g) + 1⁄2O2(g)
is rather explosive, yet there is still a finite equilibrium constant of 8.581×10-41 at 298 K. It’s hard to imagine how an equilibrium could exist! How could there be any hydrogen or oxygen gas left over the bang?
a. To understand what is going on, first fill out the remaining entries of the table of mole fractions below like in the example from question 1. Let’s assume the pressure is maintained at a constant 1 bar, as such we don’t need to worry about partial pressures etc.
b. Using the data above please write the expression for ?? = [(XH2) (Xo2 )^1/2 ] / XH2o using
Transcribed Image Text:Amount at equilibrium
Mole fractions
H₂O
n(1-a)
0₂
H₂
na
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