The value of K sp for Hg 2 Br 2 at 25°C should be calculated if the cell potential of the following galvanic cell is 1.214 V: Hg (l) | Hg 2 Br 2 (s) |Br - (0 .10M)||MnO 4 - (0 .10M),Mn 2+ (0 .10M),H + (0 .10M)|Pt (s) Concept introduction: In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with the help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and the combination of both half-reactions gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as: E cell ° = E cathode ° - E anode ° E cell ° = E reduction ° - E oxidation ° The potential of the cell can be calculated with the help of the Nernst equation that can be shown as: E° = E° cell - 0 .0592 V n log Q n = number of electrons Q = reaction quotient
The value of K sp for Hg 2 Br 2 at 25°C should be calculated if the cell potential of the following galvanic cell is 1.214 V: Hg (l) | Hg 2 Br 2 (s) |Br - (0 .10M)||MnO 4 - (0 .10M),Mn 2+ (0 .10M),H + (0 .10M)|Pt (s) Concept introduction: In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with the help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and the combination of both half-reactions gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as: E cell ° = E cathode ° - E anode ° E cell ° = E reduction ° - E oxidation ° The potential of the cell can be calculated with the help of the Nernst equation that can be shown as: E° = E° cell - 0 .0592 V n log Q n = number of electrons Q = reaction quotient
Solution Summary: The author explains how the cell potential of a galvanic cell can be calculated with the help of electrode reduction potential values. The reaction at each electrode is called as half-reaction.
Definition Definition Study of chemical reactions that result in the production of electrical energy. Electrochemistry focuses particularly on how chemical energy is converted into electrical energy and vice-versa. This energy is used in various kinds of cells, batteries, and appliances. Most electrochemical reactions involve oxidation and reduction.
Chapter 19, Problem 19.116SP
Interpretation Introduction
Interpretation:
The value of Ksp for Hg2Br2 at 25°C should be calculated if the cell potential of the following galvanic cell is 1.214 V:
In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with the help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and the combination of both half-reactions gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as: Ecell° = Ecathode° - Eanode°Ecell° = Ereduction° - Eoxidation°
The potential of the cell can be calculated with the help of the Nernst equation that can be shown as:
E° = E°cell - 0.0592 Vn log Q n = number of electronsQ = reaction quotient
3. Name this ether correctly.
H₁C
H3C
CH3
CH3
4. Show the best way to make the ether in #3 by a
Williamson Ether Synthesis.
Start from an alcohol or phenol.
5. Draw the structure of an example of a sulfide.
1. Which one(s) of these can be oxidized with CrO3 ?
(could be more than one)
a) triphenylmethanol
b) 2-pentanol
c) Ethyl alcohol
d)
CH3
2. Write in all the product(s) of this reaction. Label them
as "major" or "minor".
2-methyl-2-hexanol
H2SO4, heat
3) Determine if the pairs are constitutional isomers, enantiomers, diastereomers, or mesocompounds.
(4 points)
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