What mass of each of the following substances can be produced in 1.0 h with a current of 15 A

What mass of each of the following substances can be...

Key Concepts

Electron Stoichiometry in Electrochemical Reactions

Every electrochemical reaction involves the transfer of a specific number of electrons per ion or molecule in the redox process. Understanding the stoichiometric ratio between electrons and the substance being produced is crucial for converting the total charge into the amount of substance formed.

Faraday's Laws of Electrolysis

This concept states that the amount of substance that is produced or consumed at an electrode during an electrochemical reaction is directly proportional to the total electric charge passed through the electrolyte. It provides a quantitative relationship between the electrical current, time, and the number of moles of electrons transferred, allowing calculation of the mass of substance produced.

Current and Time Relationship to Charge

The total electric charge can be calculated by multiplying the current (amperes) by the time (seconds) the current is applied. This relationship is essential because it links the measurable current and time to the amount of electrons available for driving the chemical reaction.

Conversion from Moles to Mass (Molar Mass)

Once the number of moles of a substance produced is determined from the electron stoichiometry and the overall charge, the molar mass of the substance is used to convert this amount from moles to grams. This conversion is fundamental in relating atomic-scale quantities to macroscopic masses.

Transcript

00:01 In this question, electrical energy is used to produce a chemical change of ions in solution to the neutral elements.

00:09 Given time of one hour, on a current of 15 amps, we're going to determine the mass of each substance produced.

00:17 To solve this problem, follow these steps.

00:21 1.

00:21 Determine the quantity of coolants of charge that pass through the solution.

00:26 2.

00:27 Determine the number of moles of electrons which was required to carry that coolant.

00:31 Of charge.

00:33 Thirdly, we're going to write the half reactions, then determine the number of molds of substance produce, and fifth determine the mass of the substance produced.

00:47 One amp is equal to one coulum per second.

00:54 So 15 amps is equal to 15 times one, which is 15 columns per second.

01:04 So total coolums of charge is equal to 15 coulums per second multiply by time.

01:22 Time is given as one hour.

01:25 You need to convert hours to seconds.

01:28 One hour is equal to 3 ,600 seconds.

01:34 So 15 times 3 ,600 is 54 ,000 columns.

01:40 One mole of electrons carries a charge of one faraday.

01:53 One faraday is equal to 96 ,485 coulumps.

02:01 So therefore 96 ,485 coulams is equal to one molar of electrons.

02:11 So therefore, 54 ,000, sorry, coulams.

02:17 Is equal to 1 divided by 96 ,485 coulams multiply by 54 ,000 coulums.

02:34 And that is equal to 0 .56 moles of electrons.

02:43 So therefore, 0 .56 moles of electrons flow through the acreuse solution.

02:49 So now we are going to go through part a.

02:56 You're going to produce cobalt from cobalt 2.

03:06 This is an aqueous solution, and this is a solid.

03:12 This carries a charge of plus 2.

03:15 This cobalt is in a neutral state, so the oxidation state is zero.

03:20 To balance this equation, the cobalt 2 cartyre needs to gain two electrons.

03:26 So each cobalt -caron requires two electrons to become a cobalt atom.

03:36 So two moles of electrons produces one mole of cobalt.

03:48 Therefore, 0 .56 moles of electrons would produce 1 divided by 2, multiply by 0 .56 ,000 ,000 ,000 ,000 ,000 ,000.

04:06 5 ,6.

04:08 This is moles of, and that is equal to 0 .28 moles of cobalt was produced.

04:21 The molar mass of cobalt is equal to 58 .933195 grams per mole.

04:38 So therefore, mass of cobalts produced is equal to number of moles, which is 0 .28 moles, multiply by the molar mass, which is 58 .933195 grams per mole, and that is equal to 16 .5 grams.

05:14 Therefore, 16 .5 grams of cobalds was produced.

05:20 Now we're moving on to part b.

05:25 We have half anium iron and produce half -oam atom.

05:37 So balance this equation, half -nam catio needs to gain four electrons to become a half -nium atom.

05:51 So each mole of hafam ion requires four moles of electrons to become a half -nium atom.

06:03 So therefore four moles of electrons produces one mole of hafam.

06:12 Therefore, 0 .56 moles of electrons would produce 1 divided by 4, multiply by 0 .56 moles of electrons would produce 1 divided by 4, multiply by 0 .5 ,000.

06:25 0 .56 moles of hafonyam, and that is equal to 0 .14 moles of hafonym was produced.

06:44 Molar mass of hafonym is equal to 178 .49 grams per mole.

07:01 Therefore, the mass of hafonyam produced is equal to 0 .1 .1 .4 mou...

Please give Ace some feedback