Compute the standard cell potential for the spontaneous reaction (ie. where Sr(s) is being oxidized) at 25 °C. O 3.24 V O 8.02 V O 2.56 V O 3.24 V
Compute the standard cell potential for the spontaneous reaction (ie. where Sr(s) is being oxidized) at 25 °C. O 3.24 V O 8.02 V O 2.56 V O 3.24 V
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 29E: For the standard cell potentials given here, determine the ?G for the cell in k].. (a) 0.000V,n=2...
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If a voltaic cell is created between a Sr2+/Sr electrode and a In3+/In electrode
![Compute the standard cell potential for the spontaneous reaction (ie. where Sr(s) is being oxidized) at 25 °C.
O 3.24 V
O 8.02 V
O 2.56 V
O 3.24 V](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd6697c79-d5f6-4965-ae9d-6d22c21a2cac%2Fe92593f9-de2e-43f8-8511-9444d2e31ae1%2Fzkv7hdl_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Compute the standard cell potential for the spontaneous reaction (ie. where Sr(s) is being oxidized) at 25 °C.
O 3.24 V
O 8.02 V
O 2.56 V
O 3.24 V
![Consider the following table of standard electrode potentials
Standard Electrode Potentials at 25 °C
Reduction Half-Reaction
E° (V)
Au" (aq) + 3e
Ag (aq) + e
Fe" (ag) + 3e
» Au(s)
1.50
Ag(s)
0.80
→ Fe(s)
→ Sn(s)
-0.04
Sn** (aq) + 2e
-0.14
V*(aq) + 3e
» V(s)
-0.26
In" (aq) + 3e
Eu* (aq) + 3e → Eu(s)
→ In(s)
- 0.34
- 0.35
Cr* (aq) + 3e
Та" (aq) + Зе
Zn" (aq) + 2e
Nb" (aq) + 3e
Ti* (aq) + 2e
Al* (aq) + 3e
» Cr(s)
-0.42
» Ta(s)
-0.60
→ Zn(s)
→ Nb(s)
-0.76
-1.10
→ Ti(s)
-1.63
» Al(s)
-1.66
Be* (aq) + 2e
Am* (aq) + 2e
Pr* (aq) + 2e
Mg*(aq) + 2e
→ Be(s)
→ Am(s)
-1.85
-1.90
» Pr(s)
- 2.00
→ Mg(s)
→ Na(s)
-2.37
Na (aq) +
-2.71
Ca (aq) + 2e
Sr* (aq) + 2e
Ва (аq) + 2e
- 2.87
- 2.90
→ Ca(s)
» Sr(s)
→ Ba(s)
-2.91](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd6697c79-d5f6-4965-ae9d-6d22c21a2cac%2Fe92593f9-de2e-43f8-8511-9444d2e31ae1%2F7bvh7ii_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Consider the following table of standard electrode potentials
Standard Electrode Potentials at 25 °C
Reduction Half-Reaction
E° (V)
Au" (aq) + 3e
Ag (aq) + e
Fe" (ag) + 3e
» Au(s)
1.50
Ag(s)
0.80
→ Fe(s)
→ Sn(s)
-0.04
Sn** (aq) + 2e
-0.14
V*(aq) + 3e
» V(s)
-0.26
In" (aq) + 3e
Eu* (aq) + 3e → Eu(s)
→ In(s)
- 0.34
- 0.35
Cr* (aq) + 3e
Та" (aq) + Зе
Zn" (aq) + 2e
Nb" (aq) + 3e
Ti* (aq) + 2e
Al* (aq) + 3e
» Cr(s)
-0.42
» Ta(s)
-0.60
→ Zn(s)
→ Nb(s)
-0.76
-1.10
→ Ti(s)
-1.63
» Al(s)
-1.66
Be* (aq) + 2e
Am* (aq) + 2e
Pr* (aq) + 2e
Mg*(aq) + 2e
→ Be(s)
→ Am(s)
-1.85
-1.90
» Pr(s)
- 2.00
→ Mg(s)
→ Na(s)
-2.37
Na (aq) +
-2.71
Ca (aq) + 2e
Sr* (aq) + 2e
Ва (аq) + 2e
- 2.87
- 2.90
→ Ca(s)
» Sr(s)
→ Ba(s)
-2.91
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