How long will it take to plate out each of the following with a current of 100.0 A ? a. 1.0 kg

step 1 So we have given here three parts. First of all we will calculate the moles for aluminium. So nu

How long will it take to plate out each of the following...

Key Concepts

Faraday's Law of Electrolysis

This law relates the amount of substance produced at an electrode in an electrolytic cell to the quantity of electricity (charge) passed through the system. It asserts that the mass of the deposited substance is directly proportional to the total charge, allowing one to calculate deposition time by converting mass into moles and then using stoichiometry to establish the needed charge.

Charge and Current Relationship

In electrochemistry, current is defined as the rate of flow of electric charge. The relationship Q = I × t, where Q is charge, I is current, and t is time, is fundamental for determining how long it will take to deposit a given amount of metal given a constant current, by calculating the total charge needed and dividing by the current.

Faraday Constant

The Faraday constant represents the charge of one mole of electrons, approximately 96485 coulombs per mole. It is essential for converting between the moles of electrons involved in an electrochemical reaction and the total electric charge required for a deposition process, thereby linking chemical quantities with electrical measures.

Molar Conversions

Molar conversion involves converting between mass, moles, and number of entities using the molar mass of a substance. In electrolysis problems, this concept is utilized to convert a given mass of a metal to the corresponding number of moles, facilitating the use of stoichiometry to relate chemical reactions with the flow of electrons.

Electrochemical Stoichiometry

This concept deals with the mole ratios between reactants and electrons in an electrochemical reaction. It is crucial in determining the number of electrons required to deposit a specific amount of a substance, as different ions may require different numbers of electrons per ion to be reduced, affecting the overall calculation of the charge and time required for deposition.

Transcript

00:01 So we have given here three parts.

00:01 First of all we will calculate the moles for aluminium.

00:05 So number of moles of aluminium that's equal to we have here given mass.

00:18 So that given mass is 1 .00 kilogram.

00:21 This should be converted into grams.

00:24 So 1 kilogram consists of 1 ,000 gram and this will be multiplied by we have here.

00:32 1 mole of aluminum and divided by 27 gram of aluminum.

00:37 This is because the molar mass for aluminum is 27 gram per mole.

00:41 So this means that 1 mole of aluminum has 27 gram of aluminum.

00:45 So solving this we will have 37 .04.

00:51 So that much moles of aluminum.

00:55 Okay.

00:56 Now we have an aluminum 3 positive iron right.

01:00 So it will gain 3 electrons to form.

01:03 Al 3 this is al atom so this means that each aluminum ion requires three electrons to become aluminum atom okay so now i can calculate the number of moles of electrons so number of moles of electrons so that will be equal to we have 37 .04 4 mole of aluminum multiplied by 3 electrons right so this will be overall equals to 111 .12 mole of electron okay so now with the help of that i can calculate the amount of charge so charge passed so this will be equal to so here i i have 111 .12 mole of electron, right? so this will be multiplied by 96485 of charge divided by one mole electron.

02:28 This means that since one mole, so that's one mole of electron, that's equal to this much amount of charge, okay? so, solving this, we can find out that 10 .72 multiplying 10 raise to power 6 coulamps.

02:51 This is the amount of charge in coulamps.

02:55 Okay, now i have given current.

02:57 With the help of current, i can calculate the time because i have calculated charge here.

03:02 And since i know that time, so that will be equal to this charge q divided by i.

03:13 Okay.

03:13 I hope you know that there is a relation between charge current and time that is charge q is equal to it.

03:24 So with the help of that i have this relation putting the values...

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