1. The following oxidation and reduction half-reactions are possible for the electrolysis of potassium iodide solution. The solution contains water molecules, potassium ions (K*), and iodide ions (I-). 2H,0(1) 0,(g) + 4H*(aq) + 4e- 2H,O(1) + 2e- → H,(g) + 20H (aq) K*(aq) + e- → K(s) 21-(aq) L(s) + 2e- a. What product was formed at the anode in the electrolysis of potassium iodide solution? Explain, citing specific evi- dence from your observations. O29)+H* cael +4c-→ 2HzOce) Izca) is produced Anode the anede The confor E'ceu =+ 1.23 V product of I at by color change from Yellow to black Lobserved in the presence of starch) E'eell = to.SYV b. What product was formed at the cathode in the electrolysis of potassium iodide solution? Explain based on your observations. ZA20 1D + 2e- -> Hz lg) + 204 cag) A219) t 2014 ions are Produced k*cap)te> Kes) Hydvogen gas bubbles out from the solutio E cell = :13V and hy droxi'des turn fhe Phenolphthalein E cell = - 2.93 V to pink Solotion c. Write the balanced chemical equation for the overall redox reaction in the electrolysis of aqueous potassium iodide. Hint: Remember to balance the electrons!
1. The following oxidation and reduction half-reactions are possible for the electrolysis of potassium iodide solution. The solution contains water molecules, potassium ions (K*), and iodide ions (I-). 2H,0(1) 0,(g) + 4H*(aq) + 4e- 2H,O(1) + 2e- → H,(g) + 20H (aq) K*(aq) + e- → K(s) 21-(aq) L(s) + 2e- a. What product was formed at the anode in the electrolysis of potassium iodide solution? Explain, citing specific evi- dence from your observations. O29)+H* cael +4c-→ 2HzOce) Izca) is produced Anode the anede The confor E'ceu =+ 1.23 V product of I at by color change from Yellow to black Lobserved in the presence of starch) E'eell = to.SYV b. What product was formed at the cathode in the electrolysis of potassium iodide solution? Explain based on your observations. ZA20 1D + 2e- -> Hz lg) + 204 cag) A219) t 2014 ions are Produced k*cap)te> Kes) Hydvogen gas bubbles out from the solutio E cell = :13V and hy droxi'des turn fhe Phenolphthalein E cell = - 2.93 V to pink Solotion c. Write the balanced chemical equation for the overall redox reaction in the electrolysis of aqueous potassium iodide. Hint: Remember to balance the electrons!
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:1. The following oxidation and reduction half-reactions are possible for the electrolysis of potassium iodide solution. The
solution contains water molecules, potassium ions (K*), and iodide ions (I-).
2H,O(1)
0,(g) + 4H*(aq) + 4e-
2H,0(1) + 2e- →
H,(g) + 20H-(aq)
>
K*(aq) + e- -→ K(s)
21-(aq)
L(s) + 2e-
a. What product was formed at the anode in the electrolysis of potassium iodide solution? Explain, citing specific evi-
dence from
observations.
your
Ozg) +H* cag) +4c-→ 2 H20ee)
Izca) is produced
Anode
the anode
conforms
E'eeu = + 1.23 v
The product of Iz at
by color change from Yellow to black
Cobserved in the presence of starcn)
E cell - to.SYV
b. What product was formed at the cathode in the electrolysis of potassium iodide solution? Explain based on your
observations.
2H20 D + le- -> Hzlg) + 20H caq)
A219) $ 204- ions are ProdUced
k
caq) te--> K cs)
E cel
Hydrogen gas bubbles out fcom
solution
the
E cel
- 13 V
and hv droxides
turn the Phenolphthalein
= - 2.93 v
Solotion
to pink
c. Write the balanced chemical equation for the overall redox reaction in the electrolysis of aqueous potassium iodide.
Hint: Remember to balance the electrons!
21+ c t 2014 (89) + Hz la) +I 2a )
Transcribed Image Text:2. Using Question #1 as a guide: (a) Identify the products that were formed at the anode and the cathode in the electrolysis of
sodium chłoride solution, giving the specific evidence for their formation. (b) Write the balanced chemical equation for the
overall redox reaction.
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