Electrochemistry
Problem Example 1
Find the standard potential of the cell
Solution: The net reaction corresponding to this cell will be
- Reference Electrodes
In most electrochemical experiments our interest is concentrated on only one of the electrode reactions. Since all measurements must be on a complete cell involving two electrode systems, it is common practice to employ a reference...
- Galvanic Cells
This arrangement is called a Galvanic cell. A typical cell might consist of two pieces of metal, one zinc and the other copper, each immersed each in a solution containing a dissolved salt of the corresponding metal. The two...
- Electrochemistry
Learning Objectives(a) describe and explain redox processes in terms of electron transfer and/or of changes in oxidation number (oxidation state) (b) define the terms: (i) standard electrode (redox) potential (ii)...
- How To Balance Ionic Equations In Alkaline Medium?
(I) Standard Electrode Potential What information can we obtain from SEP? Sign – oxidation or reduction favoured Magnitude – the extent the reaction is favoured How to measure SEP? - connecting the redox couple (half cell) to SHE. - learn to draw...
- Electrochemistry : 10.1 Galvanic Cell (continued)
SPONTANEOUS REACTION occurs as the result of different ability of metal to give up their electron to flow through the circuit. CELL POTENTIAL (ECell) different in electrical potential of electrodes also called voltage or electromotive...
Electrochemistry
Standard half-cell potentials
Problem Example 1
Find the standard potential of the cell
Cu(s) | Cu2+ || Cl– | AgCl(s) | Ag(s)
and predict the direction of electron flow when the two electrodes are connected.Solution: The net reaction corresponding to this cell will be
2 Ag(s) + 2 Cl–(aq) + Cu2+(aq) → AgCl(s) + Cu(s)
Since this involves the reverse of the AgCl reduction, we must reverse the corresponding half-cell potential:Ecell = (.337 – .222) v = .115 v
Since this potential is positive, tthe reaction will proceed to the right; electrons will be withdrawn from the copper electrode and flow through the external circuit into the silver electrode. Note carefully that in combining these half-cell potentials, we did not multiply E° the for the Cu2+/Cu couple by two. The reason for this will be explained later.
- Reference Electrodes
In most electrochemical experiments our interest is concentrated on only one of the electrode reactions. Since all measurements must be on a complete cell involving two electrode systems, it is common practice to employ a reference...
- Galvanic Cells
This arrangement is called a Galvanic cell. A typical cell might consist of two pieces of metal, one zinc and the other copper, each immersed each in a solution containing a dissolved salt of the corresponding metal. The two...
- Electrochemistry
Learning Objectives(a) describe and explain redox processes in terms of electron transfer and/or of changes in oxidation number (oxidation state) (b) define the terms: (i) standard electrode (redox) potential (ii)...
- How To Balance Ionic Equations In Alkaline Medium?
(I) Standard Electrode Potential What information can we obtain from SEP? Sign – oxidation or reduction favoured Magnitude – the extent the reaction is favoured How to measure SEP? - connecting the redox couple (half cell) to SHE. - learn to draw...
- Electrochemistry : 10.1 Galvanic Cell (continued)
SPONTANEOUS REACTION occurs as the result of different ability of metal to give up their electron to flow through the circuit. CELL POTENTIAL (ECell) different in electrical potential of electrodes also called voltage or electromotive...