Question

is trying to plate gold onto his silver ring. He constructs an electrolytic cell using his ring as one of the electrodes. He runs this cell for 94.6 minutes at 224.8 mA. How many moles of electrons were transferred in this process

Answer 1

0.013 mole.

Step-by-step explanation:

From the question given above, the following data were obtained:

Time (t) = 94.6 mins

Current (I) = 224.8 mA.

Mole of electrons (e) =?

Next, we shall convert 94.6 mins to seconds. This is illustrated below:

1 min = 60 s

Therefore,

94.6 mins = 94.6 min × 60 s / 1 min

94.6 mins = 5676 s

Thus, 94.6 mins is equivalent to 5676 s.

Next, we shall convert 224.8 mA to ampere (A). This can be obtained as follow:

1 mA = 1×10¯³ A

Therefore,

224.8 mA = 224.8 mA × 1×10¯³ A / 1 mA

224.8 mA = 0.2248 A

Thus, 224.8 mA is equivalent to 0.2248 A.

Next, we shall determine the quantity of electricity flowing in circuit. This can be obtained as follow:

Time (t) = 5676 s

Current (I) = 0.2248 A

Quantity of electricity (Q) =?

Q = it

Q = 0.2248 × 5676

Q = 1275.96 C

Finally, we shall determine the mole of electron by converting the quantity of electricity (i.e 1275.96 C) to number of electrons. This can be obtained as follow:

96500 C = 1 e

Therefore,

1275.96 C = 1275.96 C × 1 e / 96500 C

96500 C = 0.013 e

Thus, the mole of electron trasfered in the process is 0.013 mole.