Electroc 908 Chapter 17| Electrochen Selected Standard Reduction Potentials at 25 °C E° (V) Half-Reaction 2+(aq) + 2e – 2Hg(l) Hg2 +0.7973 +0.771 - Fe+(aq) Fe 3+(aq) +e MnO2(s) + 40H¯(aq) +0.558 MnO4 (aq)+ 2H, O(1) + 3e¯ → I(s) + 2e 21¯(aq) +0.5355 NiO2(s) + 2H2 O() + 2e Ni(OH)2(s) + 20H¯(aq) Cu2+(aq) + 2e → Cu(s) )2 Table 17 +0.49 +0.34 +0.26808 Example 17.4 Hg2 Cl2(s) + 2e → 2Hg(l) + 2C1¯(aq) +0.22233 Calculating AgCl(s) + e - Ag(s) + Cl (aq) What is the stand +0.151 4+ → Sn+(aq) Sn**(aq) + 2e- - Solution 0.00 → H2(8) The cell in Figu 2H*(aq) + 2e and reduction of -0.1262 Pb2+(aq) + 2e → Pb(s) -0.1375 2+ Sn+(aq) + 2e → Sn(s) -0.257 Ni2+(aq) + 2e → Ni(s) The standard c -0.28 Co2*(aq) + 2e- Co(s) -0.3505 PbSO4(s) + 2e Pb(s) + SO42-(ag) boe -0.4030 Cd2+(aq) + 2e → Cd(s) Check You Fe+(aq) + 2e 2+ → Fe(s) -0.447 What is the .3+ -0.744 lead half-ce Cr(aq) + 3e → Cr(s) 2+ -1.185 Mn-(aq) + 2e → Mn(s) Intrepretir Zn(OH)2(s) + 2eT Zn(s) + 20H (aq) -1.245 Thinking caref change present of copper by a in Example Zn*(aq) + 2e → Zn(s) 2+ -0.7618 3+ Al(aq) + 3e → Al(s) -1.662 nonspontaneo ("strength") v one exhibiting Mg²(aq) + 2e- → Mg(s) -2.372 Na*(aq) + e¯ -2.71 processes, ar (hence increa potentials ar is a weaker Na(s) 2+ Ca(aq) + 2e → Ca(s) -2.868 Table 17.1 Applying th Lelde This OpenStax book is available for free at httnll
Electroc 908 Chapter 17| Electrochen Selected Standard Reduction Potentials at 25 °C E° (V) Half-Reaction 2+(aq) + 2e – 2Hg(l) Hg2 +0.7973 +0.771 - Fe+(aq) Fe 3+(aq) +e MnO2(s) + 40H¯(aq) +0.558 MnO4 (aq)+ 2H, O(1) + 3e¯ → I(s) + 2e 21¯(aq) +0.5355 NiO2(s) + 2H2 O() + 2e Ni(OH)2(s) + 20H¯(aq) Cu2+(aq) + 2e → Cu(s) )2 Table 17 +0.49 +0.34 +0.26808 Example 17.4 Hg2 Cl2(s) + 2e → 2Hg(l) + 2C1¯(aq) +0.22233 Calculating AgCl(s) + e - Ag(s) + Cl (aq) What is the stand +0.151 4+ → Sn+(aq) Sn**(aq) + 2e- - Solution 0.00 → H2(8) The cell in Figu 2H*(aq) + 2e and reduction of -0.1262 Pb2+(aq) + 2e → Pb(s) -0.1375 2+ Sn+(aq) + 2e → Sn(s) -0.257 Ni2+(aq) + 2e → Ni(s) The standard c -0.28 Co2*(aq) + 2e- Co(s) -0.3505 PbSO4(s) + 2e Pb(s) + SO42-(ag) boe -0.4030 Cd2+(aq) + 2e → Cd(s) Check You Fe+(aq) + 2e 2+ → Fe(s) -0.447 What is the .3+ -0.744 lead half-ce Cr(aq) + 3e → Cr(s) 2+ -1.185 Mn-(aq) + 2e → Mn(s) Intrepretir Zn(OH)2(s) + 2eT Zn(s) + 20H (aq) -1.245 Thinking caref change present of copper by a in Example Zn*(aq) + 2e → Zn(s) 2+ -0.7618 3+ Al(aq) + 3e → Al(s) -1.662 nonspontaneo ("strength") v one exhibiting Mg²(aq) + 2e- → Mg(s) -2.372 Na*(aq) + e¯ -2.71 processes, ar (hence increa potentials ar is a weaker Na(s) 2+ Ca(aq) + 2e → Ca(s) -2.868 Table 17.1 Applying th Lelde This OpenStax book is available for free at httnll
Electroc 908 Chapter 17| Electrochen Selected Standard Reduction Potentials at 25 °C E° (V) Half-Reaction 2+(aq) + 2e – 2Hg(l) Hg2 +0.7973 +0.771 - Fe+(aq) Fe 3+(aq) +e MnO2(s) + 40H¯(aq) +0.558 MnO4 (aq)+ 2H, O(1) + 3e¯ → I(s) + 2e 21¯(aq) +0.5355 NiO2(s) + 2H2 O() + 2e Ni(OH)2(s) + 20H¯(aq) Cu2+(aq) + 2e → Cu(s) )2 Table 17 +0.49 +0.34 +0.26808 Example 17.4 Hg2 Cl2(s) + 2e → 2Hg(l) + 2C1¯(aq) +0.22233 Calculating AgCl(s) + e - Ag(s) + Cl (aq) What is the stand +0.151 4+ → Sn+(aq) Sn**(aq) + 2e- - Solution 0.00 → H2(8) The cell in Figu 2H*(aq) + 2e and reduction of -0.1262 Pb2+(aq) + 2e → Pb(s) -0.1375 2+ Sn+(aq) + 2e → Sn(s) -0.257 Ni2+(aq) + 2e → Ni(s) The standard c -0.28 Co2*(aq) + 2e- Co(s) -0.3505 PbSO4(s) + 2e Pb(s) + SO42-(ag) boe -0.4030 Cd2+(aq) + 2e → Cd(s) Check You Fe+(aq) + 2e 2+ → Fe(s) -0.447 What is the .3+ -0.744 lead half-ce Cr(aq) + 3e → Cr(s) 2+ -1.185 Mn-(aq) + 2e → Mn(s) Intrepretir Zn(OH)2(s) + 2eT Zn(s) + 20H (aq) -1.245 Thinking caref change present of copper by a in Example Zn*(aq) + 2e → Zn(s) 2+ -0.7618 3+ Al(aq) + 3e → Al(s) -1.662 nonspontaneo ("strength") v one exhibiting Mg²(aq) + 2e- → Mg(s) -2.372 Na*(aq) + e¯ -2.71 processes, ar (hence increa potentials ar is a weaker Na(s) 2+ Ca(aq) + 2e → Ca(s) -2.868 Table 17.1 Applying th Lelde This OpenStax book is available for free at httnll
Use information from Table 17.1 (pp. 907-909 of your textbook) to answer this question. Which metal, when placed in a Co(NO3)2(aq) solution, will start a spontaneous redox reaction?
Group of answer choices
chromium (Cr)
nickel (Ni)
tin (Sn)
copper (Cu)
Transcribed Image Text:Electroc
908
Chapter 17| Electrochen
Selected Standard Reduction Potentials at 25 °C
E° (V)
Half-Reaction
2+(aq) + 2e – 2Hg(l)
Hg2
+0.7973
+0.771
- Fe+(aq)
Fe
3+(aq) +e
MnO2(s) + 40H¯(aq)
+0.558
MnO4 (aq)+ 2H, O(1) + 3e¯ →
I(s) + 2e 21¯(aq)
+0.5355
NiO2(s) + 2H2 O() + 2e Ni(OH)2(s) + 20H¯(aq)
Cu2+(aq) + 2e → Cu(s)
)2 Table 17
+0.49
+0.34
+0.26808
Example 17.4
Hg2 Cl2(s) + 2e → 2Hg(l) + 2C1¯(aq)
+0.22233
Calculating
AgCl(s) + e - Ag(s) + Cl (aq)
What is the stand
+0.151
4+
→ Sn+(aq)
Sn**(aq) + 2e- -
Solution
0.00
→ H2(8)
The cell in Figu
2H*(aq) + 2e
and reduction of
-0.1262
Pb2+(aq) + 2e → Pb(s)
-0.1375
2+
Sn+(aq) + 2e → Sn(s)
-0.257
Ni2+(aq) + 2e → Ni(s)
The standard c
-0.28
Co2*(aq) + 2e-
Co(s)
-0.3505
PbSO4(s) + 2e
Pb(s) + SO42-(ag)
boe
-0.4030
Cd2+(aq) + 2e
→ Cd(s)
Check You
Fe+(aq) + 2e
2+
→ Fe(s)
-0.447
What is the
.3+
-0.744
lead half-ce
Cr(aq) + 3e → Cr(s)
2+
-1.185
Mn-(aq) + 2e
→ Mn(s)
Intrepretir
Zn(OH)2(s) + 2eT
Zn(s) + 20H (aq)
-1.245
Thinking caref
change present
of copper by a
in Example
Zn*(aq) + 2e → Zn(s)
2+
-0.7618
3+
Al(aq) + 3e → Al(s)
-1.662
nonspontaneo
("strength") v
one exhibiting
Mg²(aq) + 2e-
→ Mg(s)
-2.372
Na*(aq) + e¯
-2.71
processes, ar
(hence increa
potentials ar
is a weaker
Na(s)
2+
Ca(aq) + 2e
→ Ca(s)
-2.868
Table 17.1
Applying th
Lelde
This OpenStax book is available for free at httnll
Definition Definition Chemical reactions involving both oxidation and reduction processes. During a redox reaction, electron transfer takes place in such a way that one chemical compound gets reduced and the other gets oxidized.
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