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

step 1 So we need to determine the mass of A. We have cobalt. We can get cobalt from acous cobalt ions.

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

Key Concepts

Faraday's Law of Electrolysis

This law relates the amount of substance transformed during electrolysis to the total electrical charge passed through the electrolyte. It states that the amount of material produced at an electrode is proportional to the total charge, which is calculated by multiplying the current by the time, and that the conversion factor involves the Faraday constant (approximately 96485 coulombs per mole of electrons).

Current and Time Relationship

This concept explains that the total charge (Q) passing through an electrolytic cell is the product of the current (I) and the time (t) for which the current flows. In calculations, ensuring consistency in units (such as converting time to seconds) is crucial for determining the total electric charge involved in the electrolysis process.

Electrode Reaction Stoichiometry

In electrolysis problems, each ion requires a specific number of electrons (n) for its reduction to the elemental form. This stoichiometric relationship is central to determining how many moles of electrons are needed to produce one mole of the substance, and it varies with the ionic charge of the species being reduced.

Mole-Mass Conversion

Once the number of moles of the substance produced is determined from the electrochemical calculations, the mass can be calculated using the substance's molar mass. This conversion is essential to translate the quantity of electricity passed into a tangible mass of material produced during electrolysis.

Transcript

00:01 So we need to determine the mass of a.

00:05 We have cobalt.

00:07 We can get cobalt from acous cobalt ions.

00:14 Then b, we need to find iodine, okay.

00:23 Mass of iodine from potassium iodide.

00:29 C we need to find the mass of hafnium from.

00:37 From acuas hafmium okay and d we need to find the mass of chromium from molten chromium oxide because molten liquid okay so for cobalts we know that the relative atomic mass of this is 58 .0 .93 okay point point gram per more all right and then the time we're given time to be one hour so that means it's going to get the time in seconds all right which should be equal to 3 ,600 seconds then we're given current to be current is 15 amperes okay there's a lot of current right so i won't first off to get the mass of this you're going to to to to you know the current multiply by time to you know to get us charge in columns okay then i'm going to multiply that by you know one more one more of of electron developed by the faradis constant which is 96 ,000 485 485 amper second is going to cancel ampers per second here is charge okay also we're going to multiply that by, you know, one mole of cobalt.

02:30 We're going to lose for cobalt.

02:35 We're going to there are two electrons here, okay? we're going to multiply by the two electrons here.

02:42 Two modes of electrons.

02:44 Also going to multiply that by the relative atomic mass of cobalt, which is 58 .93 here.

02:54 58 23 grams per mole i divide by one mole okay so you're going to get some or the mass per one mole okay and this is going to give us 16 grams of cobalt so this is what we're going to deposit using this current okay so b part be part of this is a be part of this we're going to calculate the mass of iodine from potassium iodide okay and also the reaction here we got you know iodine ram of iodine is 253 253.

03:45 253.

03:46 353 .3 .m.

03:48 So we're going to use the same formula here.

03:52 We're going to get first 15.

03:56 Current multiply by time, multiplied by one mole of electron...

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