1il66 lille6 M = O,75-X Lケっコこ1 somol _0O,7SMX=OSEM K = [NH,]< [H.]° [N] HSJ=2x= =2HFL9) ( जजा) (o.৮) 0,75 9.3125 Mores HI =0:421 9.75-x 0,75-X dx 3とmo = (ax)? 3) What would happen to the values you calculated for Kc in the experiment if the こ49 (0.75-Y Beer's Law constant (k) value you ușed was high (e.g. you used 6,000 M²' when the actual constant had a value of 5,000 M-1)? Explain your answer. २८ ccLa Ka ck As me スっ calculeired acreal, me caliu usl also be smaue cencentrat 3 smalles man me equalib Ka oum constant a crial man me eq uilibnum con stant constant dircry de substance equalibum conunmamn of me f a lower Been's con stant of on me Ca give value hrznn value ralue equalosmum con Sren PINKA in General Chemistry II Lab Manual, 2019 Revision Mimin 69 Determination of an Equilibrium Constant 35 Objectives: 1) To review Beer's Law and use it to determine the concentration of a complex involved in a chemical equilibrium. 2) To use experimental data to determine an equilibrium constant Background: de anou By now you have had experience viewing what happens during chemical reactions. Many of the reactions we've studied so far in lab go to completion. In other words, when the reaction has finished, it is assumed that the reaction has gone as far as it can, consuming at least one reactant completely. It would be more realistic to say that often chemical reactions do not go to the point that one or more reactants are consumed completely. Instead we see that a certain amount of product forms, and the forward progress of the reaction comes to a halt. This is not because the reaction stops, but because the reverse reaction is taking place at the same rate as the forward reaction. In other words, equilibrium is established. At equilibrium, the concentrations of reactants and products in a reaction will not change unless something is changed. We can express the equilibrium in mathematical terms through an equilibrium constant, which accounts for all products and reactants in solution. a A tbB >c(( +dD sc( +dD In this lab you will be looking at the equilibrium: Fe3++SCN= Fe(SCN)2+. Kea = C^ Dd The equilibrium constant expression for this reaction is: monancanCor vanes WIT products + reactans magnn Both the iron(III) cation (Fe3*) and the thiocyanate anion (SCN') are colorless in acidic [Fe(SCN)2+] [Fe3+][SCN=] Keg-7 Ke how much formed ramo solution, while the thiocyanato iron(III) complex (Fe(SCN)²*)is a deep red. The eguilibrium concentration of the complex can therefore be determined by using Beer's Law while the equilibrium concentrations of the reactants can be determined by difference if the initial concentrations before equilibrium are known. Beer's Law states that the absorbance of a solution containing a colored species is directly proportional to the concentration of the colored species. Baen's This relationship can be rewritten as an equation by placing a constant into the equation. The constant is known as absorptivity or molar absorptivity. A kC =Reo m= Absonb mmy と2m-l (Note that this is a small k and is not the same as Ke!) If Beer's Law is followed, then a plot of absorbance versus concentration should give us a straight line with slope equal to absorptivity. specs Fe 31-fom fecnO,), 3 recNO,) CSCN SIN-- fom oft S

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1il66
lille6 M =
O,75-X
Lケっコこ1 somol _0O,7SMX=OSEM
K = [NH,]<
[H.]° [N]
HSJ=2x=
=2HFL9)
( जजा) (o.৮)
0,75
9.3125
Mores
HI
=0:421
9.75-x
0,75-X
dx
3とmo
= (ax)?
3) What would happen to the values you calculated for Kc in the experiment if the
こ49
(0.75-Y
Beer's Law constant (k) value you ușed was high (e.g. you used 6,000 M²' when the
actual constant had a value of 5,000 M-1)? Explain your answer.
२८
ccLa
Ka ck
As me
スっ
calculeired
acreal, me caliu
usl also be smaue
cencentrat
3 smalles
man
me
equalib
Ka
oum constant
a crial
man me
eq uilibnum con stant
constant dircry de
substance
equalibum
conunmamn of me
f a lower Been's con stant
of
on me
Ca
give
value
hrznn value
ralue
equalosmum con Sren
Transcribed Image Text:1il66 lille6 M = O,75-X Lケっコこ1 somol _0O,7SMX=OSEM K = [NH,]< [H.]° [N] HSJ=2x= =2HFL9) ( जजा) (o.৮) 0,75 9.3125 Mores HI =0:421 9.75-x 0,75-X dx 3とmo = (ax)? 3) What would happen to the values you calculated for Kc in the experiment if the こ49 (0.75-Y Beer's Law constant (k) value you ușed was high (e.g. you used 6,000 M²' when the actual constant had a value of 5,000 M-1)? Explain your answer. २८ ccLa Ka ck As me スっ calculeired acreal, me caliu usl also be smaue cencentrat 3 smalles man me equalib Ka oum constant a crial man me eq uilibnum con stant constant dircry de substance equalibum conunmamn of me f a lower Been's con stant of on me Ca give value hrznn value ralue equalosmum con Sren
PINKA
in
General Chemistry II Lab Manual, 2019 Revision
Mimin
69
Determination of an Equilibrium Constant
35
Objectives:
1) To review Beer's Law and use it to determine the concentration of a complex
involved in a chemical equilibrium.
2) To use experimental data to determine an equilibrium constant
Background:
de
anou
By now you have had experience viewing what happens during chemical reactions.
Many of the reactions we've studied so far in lab go to completion. In other words, when
the reaction has finished, it is assumed that the reaction has gone as far as it can,
consuming at least one reactant completely.
It would be more realistic to say that often chemical reactions do not go to the point that
one or more reactants are consumed completely. Instead we see that a certain amount of
product forms, and the forward progress of the reaction comes to a halt. This is not
because the reaction stops, but because the reverse reaction is taking place at the same
rate as the forward reaction. In other words, equilibrium is established.
At equilibrium, the concentrations of reactants and products in a reaction will not change
unless something is changed. We can express the equilibrium in mathematical terms
through an equilibrium constant, which accounts for all products and reactants in
solution.
a A tbB >c(( +dD
sc( +dD
In this lab you will be looking at the equilibrium:
Fe3++SCN= Fe(SCN)2+.
Kea = C^ Dd
The equilibrium constant expression for this reaction is:
monancanCor
vanes
WIT
products +
reactans
magnn
Both the iron(III) cation (Fe3*) and the thiocyanate anion (SCN') are colorless in acidic
[Fe(SCN)2+]
[Fe3+][SCN=]
Keg-7 Ke
how much
formed
ramo
solution, while the thiocyanato iron(III) complex (Fe(SCN)²*)is a deep red. The
eguilibrium concentration of the complex can therefore be determined by using Beer's
Law while the equilibrium concentrations of the reactants can be determined by
difference if the initial concentrations before equilibrium are known.
Beer's Law states that the absorbance of a solution containing a colored species is directly
proportional to the concentration of the colored species.
Baen's
This relationship can be rewritten as an equation by placing a constant into the equation.
The constant is known as absorptivity or molar absorptivity.
A kC
=Reo
m= Absonb mmy
と2m-l
(Note that this is a small k and is not the same as Ke!)
If Beer's Law is followed, then a plot of absorbance versus concentration should give us a
straight line with slope equal to absorptivity.
specs
Fe 31-fom fecnO,),
3
recNO,)
CSCN
SIN-- fom
oft S
Transcribed Image Text:PINKA in General Chemistry II Lab Manual, 2019 Revision Mimin 69 Determination of an Equilibrium Constant 35 Objectives: 1) To review Beer's Law and use it to determine the concentration of a complex involved in a chemical equilibrium. 2) To use experimental data to determine an equilibrium constant Background: de anou By now you have had experience viewing what happens during chemical reactions. Many of the reactions we've studied so far in lab go to completion. In other words, when the reaction has finished, it is assumed that the reaction has gone as far as it can, consuming at least one reactant completely. It would be more realistic to say that often chemical reactions do not go to the point that one or more reactants are consumed completely. Instead we see that a certain amount of product forms, and the forward progress of the reaction comes to a halt. This is not because the reaction stops, but because the reverse reaction is taking place at the same rate as the forward reaction. In other words, equilibrium is established. At equilibrium, the concentrations of reactants and products in a reaction will not change unless something is changed. We can express the equilibrium in mathematical terms through an equilibrium constant, which accounts for all products and reactants in solution. a A tbB >c(( +dD sc( +dD In this lab you will be looking at the equilibrium: Fe3++SCN= Fe(SCN)2+. Kea = C^ Dd The equilibrium constant expression for this reaction is: monancanCor vanes WIT products + reactans magnn Both the iron(III) cation (Fe3*) and the thiocyanate anion (SCN') are colorless in acidic [Fe(SCN)2+] [Fe3+][SCN=] Keg-7 Ke how much formed ramo solution, while the thiocyanato iron(III) complex (Fe(SCN)²*)is a deep red. The eguilibrium concentration of the complex can therefore be determined by using Beer's Law while the equilibrium concentrations of the reactants can be determined by difference if the initial concentrations before equilibrium are known. Beer's Law states that the absorbance of a solution containing a colored species is directly proportional to the concentration of the colored species. Baen's This relationship can be rewritten as an equation by placing a constant into the equation. The constant is known as absorptivity or molar absorptivity. A kC =Reo m= Absonb mmy と2m-l (Note that this is a small k and is not the same as Ke!) If Beer's Law is followed, then a plot of absorbance versus concentration should give us a straight line with slope equal to absorptivity. specs Fe 31-fom fecnO,), 3 recNO,) CSCN SIN-- fom oft S
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