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Periodic Table of the Elements
Nernst equation:
Q
n
V
E
Q
n
V
E
Q
nF
RT
E
E
log
05917
.
0
ln
025693
.
0
ln
-
°
=
-
°
=
-
°
=
(at T = 298.15K)
Arrhenius equation:
)
/
exp(
RT
E
A
k
a
-
=
Reduction half-reaction
E° (V)
ClO
4
-
+ 2H
+
+ 2 e
-
barb2right
ClO
3
-
+ H
2
O +1.23
Ag
+
+ e
-
barb2right
Ag
+0.80
Pb
2+
+ 2 e
-
barb2right
Pb
-0.13
Atomic masses
Iodine = 126.90 g/mol
Hydrogen = 1.008 g/mol
R = 1.3807E-23 J/K
N
A
= 6.022E23 particles/mol
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Chemistry 204
Practice Exam 3 – 40 minutes
1. Balance the following electrochemical equation in acidic condition using the smallest
whole-number coefficient. What is the reaction quotient (Q) for the following reaction?
Ag(s) | Ag
+
(aq) || ClO
4
-
(aq), H
+
(aq), ClO
3
-
(aq) | Pt (s), E = +0.40 V.
2. A lead electrode (cathode) in 0.010 M Pb(NO
3
)
2
(aq) is connected to a hydrogen
electrode (anode) in which the pressure of H
2
is 0.057 V at 25 °C. What is the pH of the
electrolyte at the hydrogen electrode?
3. When 0.52 g of H
2
and 0.19 g of I
2
are confined to a 750-mL reaction vessel and heated to
700 K, they react by a second-order process (first order in each reactant), with k = 0.063
L/(mol*s) in the rate law (for the rate of formation of HI). (a) What is the initial rate? (b) By
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- Spring '08
- Gruebele
- Chemistry, Periodic Table, Reaction, 5 l, 25 °C, 23 J, 6 L, 575 K
-
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