Chemistry: How long would it take to produce enough aluminum to make a case (24 cans) of aluminum soft drink cans if each can used 3 g of aluminum, a current of 5.00 x 104 A was employed, and the current efficiency was 93.9 %?

How long would it take to produce enough aluminum

Ответ:

khush77

20.01.2022

Chemistry

Answer : It takes time to produce 3 g of aluminium is, 165 seconds.

Explanation :

As we are given that the mass of aluminium is, 3 grams. Now we have to calculate the total mass of aluminum.

Total mass of aluminum = 3g × 24 = 72 g

Now we have to calculate the moles of aluminum.

$\text{Moles of Al}=\frac{\text{Mass of Al}}{\text{Molar mass of Al}}$

Molar mass of Al = 27 g/mol

$\text{Moles of Al}=\frac{72g}{27g/mol}=2.67mol$

As, 1 mole of Al has 3 Faradays

So, 2.67 mole of Al has = $2.67\times 3=80.1$ Faradays

and,

Charge = $80.1\text{ Faradays}\times \frac{96500\text{ coulombs}}{1\text{ Faradays}}=7.73\times 10^6\text{ coulombs}$

Current = $5.00\times 10^4A\times \frac{93.9}{100}=46950A$

Now we have to calculate the time.

$Time=\frac{Charge}{Current}=\frac{7.73\times 10^6}{46950}=164.6s\aaprox 165s$

Hence, it takes time to produce 3 g of aluminium is, 165 seconds.

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Ответ:

reneewilliams20

20.08.2020

Chemistry

Yet both compounds and elements are considered pure substances. Pure compounds are created when elements combine permanently, forming one substance. For example, when the elements mercury and oxygen combine, and a chemical reaction takes place, mercury (II) oxide is created.

Hope this helps!

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How long would it take to produce enough aluminum to make a case (24 cans) of aluminum soft drink cans if each can used 3 g of aluminum, a current of 5.00 x 104 A was employed, and the current efficiency was 93.9 %?

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