How many hours would it take to reduce one mole of Al+3 to aluminum using a current of 22.2 Amps? Question 12 options: A) 3.6 hours B) 13020 hours C) 217 hours D) 0.22 hours

Option (A) 3.6 hours

Explanation:

Data obtained from the question include:

Current (I) = 22.2A

Time (t) =..?

Next, we shall determine the quantity of electricity needed to reduce 1 mole of Al^3+ to aluminium metal.

This is illustrated below below:

Al^3+ + 3e —> Al

From the above equation, 3 electrons are needed to reduce 1 mole of of Al^3+ to aluminium metal.

Recall:

1e = 1 Faraday = 96500C

Therefore, 3e = 3 x 96500C = 289500C.

Therefore, 289500C of electricity is needed to reduce 1 mole of Al^3+ to aluminium metal.

Next, we shall determine the time taken for 289500C of electricity to reduce 1 mole of Al^3+ to aluminium metal using a current of 22.2A. This can be achieved as follow:

Quantity of electricity (Q) = 289500C

Current (I) = 22.2A

Time (t) =..?

Q = it

289500 = 22.2 x t

Divide both side by 22.2

t = 289500/22.2

t = 13040.5 secs.

Finally, we shall convert 13040.5 secs to hours. This is illustrated below:

3600 s = 1 hr

Therefore, 13040.5 s = 13040.5/3600 = 3.6 hrs

Therefore, the time taken for the reaction is 3.6 hours

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