Use the Standard Reduction Table provided on page 4 to answer these questions. Name one substance that: (just give one answer, even if there are several correct answers) a) can oxidize I– to I2, but cannot oxidize Br– to Br2 _______________ b) can reduce Sn2+ to Sn, but cannot reduce Co2+ to Co __________________ c) can oxidize Fe to Fe2+, but cannot oxidize Fe2+ to Fe3+ _________________
Science behind corrosion-test
Corrosion is defined as an activity that transforms refined metals into more chemically stable forms such as oxide, hydroxide, carbonate, or sulfide. It refers to the slow decomposition of things (typically metals); thanks to chemical and/or electrochemical reactions with their surroundings. Corrosion engineering is the science of preventing and controlling corrosion.
Corrosion
Corrosion is defined as an activity that transforms refined metals into more chemically stable forms such as oxide, hydroxide, carbonate, or sulfide. It refers to the slow decomposition of things (typically metals); thanks to chemical and/or electrochemical reactions with their surroundings. Corrosion engineering is the science of preventing and controlling corrosion.
Use the Standard Reduction Table provided on page 4 to answer these questions.
Name one substance that: (just give one answer, even if there are several correct answers)
a) can oxidize I– to I2, but cannot oxidize Br– to Br2 _______________
b) can reduce Sn2+ to Sn, but cannot reduce Co2+ to Co __________________
c) can oxidize Fe to Fe2+, but cannot oxidize Fe2+ to Fe3+ _________________
d) can reduce Cu2+ to Cu, but cannot reduce Pb2+ to Pb _________________
For the same table. Assume all
solutions are at 1 M concentration.
True or False?
T F a) Ce4+ is a stronger oxidizing agent than permanganate ion
T F b) If you combine cobalt metal with Fe2+ ion, a
T F c) cadmium metal will react with hydrochloric acid to make H2 gas
T F d) mercury metal will reduce Hg2+ to Hg22+
T F e) Li+ ion is a strong reducing agent
![STANDARD REDUCTION POTENTIALS
Rectangular Sip
COUPLE
ɛ°(Volts)
COUPLE
E°(Volts)
SO42-
F2
F2
S20g2-
BiO3
H2O2
PbO2
Ce4+
MnO4
ClO3
PbO2
Au³+
|Cl2
Cr20,2-
MnO2
02
Br2
HF (H+)
H2SO3 (H+)
Sn2+
+3.03
+0.20
F-
+2.87
Sn4+
+0.15
SO42-
+2.05
S
H2S (H†)
+0.141
Bi3+
+2.0
Hg2Br2
Hg (Br")
+0.140
H2O (H+)
+1.78
AgBr
Ag (Br")
+0.0713
PBSO4 (H*, SO42-).
+1.685
H+
H2
+0.0000
Ce3+
+1.61
Pb2+
Pb
-0.126
Mn2+ (H+)
+1.491
Sn2+
Sn
-0.136
CI- (H*)
Pb2+ (H*)
+1.47
AgI
Ag (I-)
-0.152
+1.46
Ni2+
Ni
-0.250
Au
+1.42
Co2+
Со
-0.277
Cl-
+1.358
In3+
In
-0.342
Cr3+ (H†)
+1.33
PBSO4
Pb (SO42-)
-0.355
Mn2+ (H+)
+1.28
Cd2+
Cd
-0.402
H2O (H*)
+1.229
Cr3+
Cr2+
-0.41
Н2 (pH — 7)
H2O
Fe2+
Br
+1.065
-0.414
NO3
Hg2+
H2O2
02
Ag+
Hg22+
Fe3+
|02
MnO4
NO (H+)
+0.96
Fe
-0.440
Hg22+
H2C2O4 (H†)
S2-
+0.910
CO2
-0.49
OH-
+0.87
S
-0.508
H2O (pH = 7)
+0.815
Cr3+
Cr
-0.71
Ag
+0.7996
Zn2+
Zn
-0.762
Hg
+0.799
H2O
Н2 (ОН")
-0.828
Fe2+
+0.771
Mn2+
Mn
-1.03
H2O2 (H†)
+0.682
A]3+
Al
-1.67
Mg2+
Mg(OH)2----
MnO2 (OH)
+0.57
Mg
-2.375
I-
+0.535
Mg (OH-)
-2.67
Cu+
Cu
+0.522
Na+
Na
-2.71
Ag2CrO4
|02
Ag (CrO42-)
+0.446
Ca2+
Ca
-2.76
Н2О (ОН)
+0.401
Sr2+
Sr
-2.89
Cu2+
Hg2Cl2
AgCl
Cu
+0.337
Ва2+
Ва
-2.90
Hg (CI)
+0.268
K+
-2.92
Ag (CI-)
+0.222
Lit
Li
-3.05](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F793c7cf3-f790-48f6-9e1d-49d8157e667b%2Fa2d992dd-5f9d-4915-9181-df16663f3177%2Fh4zeien_processed.png&w=3840&q=75)
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