Consider the following table of standard electrode potentialsStandard Electrode Potentials at 25 °CReduction Half-ReactionE" (V)Au" (ag) + ЗеAg"(aq) +Fe* (aq) + 3eSn²(aq)v*(aq) + 3eIn"(ag) + 3eEu" (ag) + 3eCr* (aq)Тa" (ag) + ЗеZn*(aq)Nb* (aq)» Au(s)1.50eAg(s)0.80» Fe(s)-0.04+ 2e» Sn(s)-0.14» V(s)-0.26» In(s)-0.34» Eu(s)-0.35+ 3e» Cr(s)-0.42» Ta(s)-0.60» Zn(s)» Nb(s)→ Ti(s)→ Al(s)» Be(s)+ 2e-0.76+ 3e-1.10Ti (aq) + 2eAl" (aq) + 3eВе (ag) + 2еAm* (ag) + 2e-1.63-1.66-1.85» Am(s)-1.90Pr* (ag) + 2e"» Pr(s)-2.00Mg* (aq) + 20- Mg(s)» Na(s)» Ca(s)-2.37Na (aq) +Ca*(aq)Sr* (aq) + 2eBa (aq)e-2.712e- 2.87» Sr(s)-2.90+ 2e+ Ba(s)-2.91 Compute the standard cell potential for the spontaneous reaction (ie. where Sr(s) is being oxidized) at 25 °C.O -2.94 VO 2.86 VO 2.94 VO 8.62 V

The standard potential of the cell also called as standard potential of electrode is basically the…

Answered: Compute the standard cell potential for…

Compute the standard cell potential for the spontaneous reaction (ie. where Sr(a) is being oxidized) at 25 °C. O 2.04 V O 2.86 V O 2.04 V 8.82 V

Fundamentals Of Analytical Chemistry

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Author:Skoog

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Chapter19: Applications Of Standard Electrode Potentials

Section: Chapter Questions

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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

Consider the following table of standard electrode potentials
Standard Electrode Potentials at 25 °C
Reduction Half-Reaction
E" (V)
Au" (ag) + Зе
Ag"(aq) +
Fe* (aq) + 3e
Sn²(aq)
v*(aq) + 3e
In"(ag) + 3e
Eu" (ag) + 3e
Cr* (aq)
Тa" (ag) + Зе
Zn*(aq)
Nb* (aq)
» Au(s)
1.50
e
Ag(s)
0.80
» Fe(s)
-0.04
+ 2e
» Sn(s)
-0.14
» V(s)
-0.26
» In(s)
-0.34
» Eu(s)
-0.35
+ 3e
» Cr(s)
-0.42
» Ta(s)
-0.60
» Zn(s)
» Nb(s)
→ Ti(s)
→ Al(s)
» Be(s)
+ 2e
-0.76
+ 3e
-1.10
Ti (aq) + 2e
Al" (aq) + 3e
Ве (ag) + 2е
Am* (ag) + 2e
-1.63
-1.66
-1.85
» Am(s)
-1.90
Pr* (ag) + 2e"
» Pr(s)
-2.00
Mg* (aq) + 20
- Mg(s)
» Na(s)
» Ca(s)
-2.37
Na (aq) +
Ca*(aq)
Sr* (aq) + 2e
Ba (aq)
e
-2.71
2e
- 2.87
» Sr(s)
-2.90
+ 2e
+ Ba(s)
-2.91

Compute the standard cell potential for the spontaneous reaction (ie. where Sr(s) is being oxidized) at 25 °C.
O -2.94 V
O 2.86 V
O 2.94 V
O 8.62 V

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