# Chem104 Quiz 5 ANSWERS Self Check Due by 5 PM Tuesday. 1

```Chem104
Self Check Due by 5 PM Tuesday.
1. The reaction:
[Cu(H2O)6]+ + Cl-  [CuCl(H2O)5]+ + H2O
has the equilibrium constant K = 0.28. 100mL of this reaction system is at
equilibrium with these concentrations
[Cu(H2O)62+] = 0.40M, [Cl-] = 7.1 M, [CuCl(H2O)5+] = 0.80 M.
and then 2.0 g LiCl is added to the 100mL of solution.
(a). What will happen to the distribution of the species in this reaction? Prove your
prediction by calculating and interpreting Q.
Addition of more Cl- to the equilibrium will push the reactants to make more
products; the equilibrium shifts right.
Calculation of new [Cl]:
(2.0 g / 42.3 g mol-1) / 0.100 L = 0.473 M Cl- added.
New [Cl-] before equilibrium is re-established 7.1 M + 0.473 M = 7.573 M
NOTE: at this point it is best to keep all the sig figs until the end. Experience
will show you this. Truncating the sig figs too soon in a Keq calc can mean
losing the answer which is often as small as the new concentrations (the “x”)
Q= [Cu-Cl[ / [Cu2+][Cl-] = 0.80 / 0.40 x 7.573 = 0.264 < Keq = 0.28.
When Q < K, the reaction shift right to make more prodcts.
(b) What are the new equilibrium concentrations established after the lithium
Create the ICEbox:
Initial
[Cu2+]
0.40 M
[Cl]
7.573 M
[Cu-Cl]
0.80 M
Change
-x
-x
+x
Equil
0.40 –x
7.573 –x
0.80 + x
Keq = 0.28 = [Cu-Cl[ / [Cu2+][Cl-] = (0.80 + x) / (0.40 –x) (7.573 –x)
0.28 (0.40 –x) (7.573 –x) = (0.80 + x)
0.848 – 2.23x - 0.28 x2 = 0.8 + x
0 = -0.048 + 3.23x + 0.28 x2
x = 0.0154
So final equilibrium concentrations are:
[Cu2+] = 0.40 - 0.0154 = 0.385 M
[Cl-] = 7.573 - 0.0154 = 7.56 M
[Cu-Cl] = 0.80 + 0.0154 = 0.815 M
(c) What is the equilibrium constant for this reaction?
[CuCl(H2O)5]+ + H2O
 [Cu(H2O)6]+ + Cl-
This reaction the reverse of the one in (a), so its K will be 1/ Keq in (a) or 1/ 0.28.
The Keq for the reaction in (c) is 3.57.
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