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In the electrolysis of a basic solution, oxygen can be produced by the half-reaction
4OH- = O2 + 2H2O + 4e-
How many moles of O2 can be produced from a solution that was electrolyzed for 3.00 hours using a current of 8.00 A?
1.49 x 10-2
4.48 x 10-2
0.224
0.448
0.896
The numerical value of the Faraday constant is given as 96,500. This value represents
the number of coloumbs of charge carried by one mole of
electrons.
the number of electrons corresponding to one coloumb of
charge.
the number of electrons corresponding to one mole of
electric charge.
the number of ions discharged by the passage of one mole
of electrons.
96,500 amp/sec.
30
60
3.2 × 103
2.7 × 104
3.7 × 10-5
is greatest in a solution of pH
1.0
3.0
7.0
10.0
13.0
Consider the following standard electrode potentials
Ag+ + e- = Ag, Eo = 0.80 V
Mn2+ + 2e- = Mn, Eo = -1.18 V
for the standard cell
Mn|Mn2+(aq)||Ag+(aq)|Ag
Which of the following statements are true?
1. The cell voltage will be 1.98 V.
2. One half-cell reaction is Mn = Mn2+ + 2e-
.
3. The overall cell potential will decrease with
time.
1 only
2 only
3 only
1 and 2 only
1, 2, and 3
positive. This means that
ΔGo is negative and
K is less than 1.
ΔGo is negative and
K is greater than 1.
ΔGo is zero and K
is greater than 1.
ΔGo is positive and
K is greater than 1.
ΔGo is positive and
K is less than 1.
Pb
Mg2+
Ag+
Ag
H2
For the reaction Cl2(g) + 2Fe2+(aq) ⇌ 2Fe3+(aq) + 2Cl-(aq) the value of Eo is 0.59 V.
The value of Eo for Fe3+(aq) + Cl-(aq) ⇌ 1/2 Cl2(g) + Fe2+(aq) is
-1.18 V
-0.59 V
-0.30 V
0.30 V
0.59 V
