0.012 mole of electron
Explanation:
From the question given above, the following data were obtained:
Time (t) = 90.6 minutes
Current (I) = 213.8 mA
Number of mole of electrons =?
Next, we shall convert 90.6 mins to seconds. This can be obtained as follow:
1 min = 60 s
Therefore,
90.6 mins = 90.6 × 60
90.6 mins = 5436 s
Next, we shall convert 213.8 mA to A. This can be obtained as follow:
1000 mA = 1 A
Therefore,
213.8 mA = 213.8 mA × 1 A / 1000 mA
213.8 mA = 0.2138 A
Next, we shall determine the quantity of electricity used in the process. This can be obtained as follow:
Time (t) = 5436 s
Current (I) = 0.2138 A
Quantity of electricity (Q) =?
Q = it
Q = 0.2138 × 5436
Q = 1162.2168 C
Next, the equation for the reaction.
Au⁺ + e —> Au
From the balanced equation above,
1 mole of electron was transferred.
Recall:
1 faraday = 96500 C = 1 e
Thus,
96500 C of electricity is needed to transfer 1 mole of electron.
Finally, we shall determine the number of mole electrons transferred by the application of 1162.2168 C of electricity. This can be obtained as follow:
96500 C of electricity is needed to transfer 1 mole of electron.
Therefore,
1162.2168 C of electricity will transfer = 1162.2168 / 96500 = 0.012 mole of electron
Thus, 0.012 mole of electron was transferred in the process.
