At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.100 M and [NO]=0.500 M....
Homework Answers
According to Le Chatelier’s principle, in a chemical reaction at equilibrium, if concentration is changed then equilibrium will shift in a direction that oppose the change in concentration. A new equilibrium is established by this change.
For a reaction,
The equilibrium constant, 
can be written as
![„[a],[v]
„la].[ɔ] – °x](http://img.homeworklib.com/questions/bfdfdec0-240c-11eb-ab0f-2b0238c33024.png?x-oss-process=image/resize,w_560)
Here
,
,
and 
are concentration of A, B , C and D respectively.
The balanced chemical equation is,
Equilibrium constant for this reaction can be written as:
![[NO]
[N][0]](http://img.homeworklib.com/questions/439e0d80-eb3c-11ea-ba0e-6b5706d13b98.png?x-oss-process=image/resize,w_560)
Now, substitute 0.500 M for 
, 0.100 M for 
and 0.100 M for 
in expression of equilibrium constant and calculate value of 
.
When more 
is added then concentration increases to 0.800 M. Then, according to Le Chatelier’s principle, the reaction will shift towards left.
Construct ICE table to calculate change in concentration.
Now, equilibrium constant for this reaction is as follow.
Substitute 
for and , 
for , 25.0 for and calculate value of x.
Now, concentration of from ICE table is as follow.
![[NO]=0.800–2x](http://img.homeworklib.com/questions/c2780b20-240c-11eb-8389-5dd1ca423e27.png?x-oss-process=image/resize,w_560)
Substitute 0.0429 for x and calculate final concentration of .
![[NO]=0.800-2(0.0429)
=0.714 M](http://img.homeworklib.com/questions/c2c091c0-240c-11eb-878a-0d8e11138446.png?x-oss-process=image/resize,w_560)
Therefore, after re-establishment of equilibrium final concentration ofis 0.714 M.
The final concentration of is 0.714 M.
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At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.100 M and [NO]=0.500 M....
At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.100 M and [NO]=0.500 M....
At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.100 M and [NO]=0.500 M. N2(g) + O2 (g) <----> 2NO(g) If more NO is added, bringing its concentration to 0.800 M, what will the final concentration of NO be after equilibrium is re-established? _____M
At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.100 M[N2]=[O2]=0.100 M and [NO]=0.600...
At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.100 M[N2]=[O2]=0.100 M and [NO]=0.600 M.[NO]=0.600 M. N2(g)+O2(g)−⇀↽−2NO(g)N2(g)+O2(g)↽−−⇀2NO(g) If more NONO is added, bringing its concentration to 0.900 M,0.900 M, what will the final concentration of NONO be after equilibrium is re‑established? [NO]final=
At equilibrium, the concentrations in this system were found to be [N2] = [O2] = 0.200 M and [NO] = 0.400 M.
At equilibrium, the concentrations in this system were found to be [N2] = [O2] = 0.200 M and [NO] = 0.400 M. N2(g) + O2(g) ⇌ 2NO(g) If more NO is added, bringing its concentration to 0.700 M, what will the final concentration of NO be after equilibrium is re-established?
At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.300 M and [NO]=0.600 M...
At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.300 M and [NO]=0.600 M N2(g)+O2(g)↽−−⇀2NO(g) If more NO is added, bringing its concentration to 0.900 M, what will the final concentration of NO be after equilibrium is re-established?
At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.300 M[N2]=[O2]=0.300 M and [NO]=0.400...
At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.300 M[N2]=[O2]=0.300 M and [NO]=0.400 M.[NO]=0.400 M. N2(g)+O2(g)−⇀↽−2NO(g)N2(g)+O2(g)↽−−⇀2NO(g) If more NONO is added, bringing its concentration to 0.700 M,0.700 M, what will the final concentration of NONO be after equilibrium is re‑established?
At equilibrium, the concentrations in this system were found to be [N,] = [0] = 0.100...
At equilibrium, the concentrations in this system were found to be [N,] = [0] = 0.100 M and (NO) = 0.600 M. NA (6) + O2() 2NO(g) If more NO is added, bringing its concentration to 0.900 M, what will the final concentration of NO be after equilibrium is re-established? (NO) =
At equilibrium, the concentrations in this system were found to be [N,] = [02] = 0.300 M and [NO] = 0.600 M. N,(g)...
At equilibrium, the concentrations in this system were found to be [N,] = [02] = 0.300 M and [NO] = 0.600 M. N,(g) + O2(g) = 2 NO(g) If more NO is added, bringing its concentration to 0.900 M, what will the final concentration of NO be after equilibrium is re-established? [NO]inal = 0.4
For the reaction 2 H2O(g) + 2 H2(g) + O2(g) the equilibrium concentrations were found to...
For the reaction 2 H2O(g) + 2 H2(g) + O2(g) the equilibrium concentrations were found to be [H,0) = 0.250 M, [H2) = 0.520 M, and [0,1 = 0.800 M. W equilibrium constant for this reaction? Kon II
Initial concentrations (M) Mixture [XY] [X] [Y] A 0.100 0 0 B 0.500 0.100 0.100 C...
Initial concentrations (M) Mixture [XY] [X] [Y] A 0.100 0 0 B 0.500 0.100 0.100 C 0.200 0.300 0.300 PART B: Based on a Kc value of 0.230 and the given data table, what are the equilibrium concentrations of XY, X, and Y, respectively? Express the molar concentrations numerically.
For the reaction 2H2O(g)−⇀↽−2H2(g)+O2(g) the equilibrium concentrations were found to be [H2O]=0.250 M, [H2]=0.340 M, and...
For the reaction 2H2O(g)−⇀↽−2H2(g)+O2(g) the equilibrium concentrations were found to be [H2O]=0.250 M, [H2]=0.340 M, and [O2]=0.750 M. What is the equilibrium constant for this reaction?
At equilibrium, the concentrations in this system were found to be [N,] = [0] = 0.100 M and (NO) = 0.600 M. NA (6) + O2() 2NO(g) If more NO is added, bringing its concentration to 0.900 M, what will the final concentration of NO be after equilibrium is re-established? (NO) =
At equilibrium, the concentrations in this system were found to be [N,] = [02] = 0.300 M and [NO] = 0.600 M. N,(g) + O2(g) = 2 NO(g) If more NO is added, bringing its concentration to 0.900 M, what will the final concentration of NO be after equilibrium is re-established? [NO]inal = 0.4
For the reaction 2 H2O(g) + 2 H2(g) + O2(g) the equilibrium concentrations were found to be [H,0) = 0.250 M, [H2) = 0.520 M, and [0,1 = 0.800 M. W equilibrium constant for this reaction? Kon II
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