question archive In an electrochemistry experiment, the cyclic voltammetry technique was applied for the identification of the potassium ferricyanide concentration (unknown compound)
In an electrochemistry experiment, the cyclic voltammetry technique was applied for the identification of the potassium ferricyanide concentration (unknown compound)
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In an electrochemistry experiment, the cyclic voltammetry technique was applied for the identification of the potassium ferricyanide concentration (unknown compound). In the liquid system, the potassium ferricyanide is converted to the potassium ferrocyanide by applying the cyclic voltammetry techniques. The oxidation peak was recorded by three replicates of experiments individual in table 1. We have an unknown concentration of potassium ferricyanide solution with three replicates of I results listed in the table 1 5.512 × 10-5 A, 5.852 × 10-5 A ?5.666 × 10-5 A. Please use the table below to calculate the concentration of the unknown compound (potassium ferricyanide). If the unknown concentration should be 7.00 mM, please carry out the propagation of error analysis.
Half-cell reaction: Fe(CN)63- + e- → Fe(CN)6 4- ----------------------------------- (1)
Table 1 the calculation worksheet for the unknown concentration of iron complex redox couple.
|
Concentration |
Ip(a) 1 /A |
Ip(a) 2/A |
Ip(a) 3/A |
Ip(a) average /A |
Standard deviation |
|
2 |
2.209 × 10-5 |
2.008 × 10-5 |
1.564 × 10-5 |
||
|
4 |
4.259 × 10-5 |
4.207 × 10-5 |
4.309 × 10-5 |
||
|
6 |
6.28 × 10-5 |
6.06 × 10-5 |
5.974 × 10-5 |
||
|
8 |
8.564 × 10-5 |
9.034 × 10-5 |
8.532 × 10-5 |
||
|
10 |
12.66 × 10-5 |
12.08 × 10-5 |
12.32 × 10-5 |
||
|
Unknown |
5.512 × 10-5 |
5.852 × 10-5 |
5.666 × 10-5 |
