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Calculate the total mass (g) of copper metal electroplated from a Cu2+ solution ran with a current of 1.23A for 73.1 minutes...

Question

Calculate the total mass (g) of copper metal electroplated from a Cu2+ solution ran with a current of 1.23A for 73.1 minutes

Calculate the total mass (g) of copper metal electroplated from a Cu2+ solution ran with a current of 1.23A for 73.1 minutes



Answers

Calculate what mass of copper could be electroplated from a CuSO solution using an electric current of $2.50 \mathrm{~A}$ for $5.00 \mathrm{~h}$. Assume 100 efficiency.

So in this question we have been asked to ask that what massive topic quickly electro plated from solution containing see You score forward And the current flowing is 2.5 empty years. 4 7.1 hours 7.1 Armors. And we can assume 100% efficiency. So we know that it will get converted into copper so it will require two electrons because it isn't too plus observation state corporation to close observation ST so 2.5 pair of electrons are getting flowed for 7.1 hours which is which is multiplied by 3600 to 7 seconds. This is the amount of electron microscope. All right now We know this is the amount of electrons and columns that are before we know that one mole of electrons contains 965 double zero Faraday's. So uh, this will give us the number of moles of electron that will flow. And now we'll divide this way to to get the final answer that how many, how many moles off properly we will get now. Well, have we have to report the uncertain mass of. So what we'll have to do is multiply this by 63.5 as this is the atomic rate of carpet to get our final answer. Right. So what we can do here is we can calculate this very easily. Now doing this war will get we can cancel this 80 And uh just give me 20 seconds to do the calculation. Yeah, yeah, yeah, Yeah. So the final answer comes out to be 21.0-4 grams of copper. so this is our and two.

In this problem, we need to use the information that we're given in order to calculate the molar mass of solid copper. We're told that we pass a current of 0.750 ants for a time length of 25 minutes and we deposit 0.369 grams of solid copper from a solution of see us So four. We know that sulphate eso four has a charge of two minus. So that must mean we start with C u two plus an inquiry, a solution. And if we end up from C u two plus two solid copper, that must mean that we reduce you to plus by adding two electrons. So that is how you know this is the equation that represents that electroplating. Now we use dimensional analysis in order to calculate the total number of moles of see you that were played it out. And we know that the molar mass is the mass divided by the moles were told the mass. It has played it out in grams. So we take the grams divided by the total number of moles. So we begin by finding the number of moles of see you that were deposited. We ran this current for 25 minutes and we need to first convert that in two seconds. We know that one minute is equal to 60 seconds and the current was 0.750 amps, which is equal to cool ums per second. And now we can multiply this by Faraday's Constant 96,000 485 cool ums where every one mole of electrons And now, based on the reduction reaction, we require two moles up electrons in order to produce one mole of solid copper. So two moles of electrons We're required to reduce every one mole of solid copper. And now, once we can't sell off, the units were left with moles of copper now comes out to about 0.0 583 moles. Now, to find the molar mass, we take the mass that we're given in grams, which is 0.369 grams of copper, divided by the number of moles that we just calculated 0.583 moles in. That gives us a final value for the more massive copper to be about 63 0.3 grams per mole

So here we're looking to perform some basic calculations fast. People starting off with a calculation for moles, she is equal to the mass divided by the molecular weight So fast we've got the copper That is equal to 7.36 grounds divided by 63.55 g per mole. That's equal to 9.1158 moles. And then the same physique That's equal to 9.51g, Divided by 65.38 g per mole. That's equal to not point not not 78 most. And so when we have 7.36 g of copper that is contaminated with 9.51 g of sink, the total mass Of the sample becomes 7.8 Seven grounds. The total moles is not .1236 moles. We just add the numbers are calculated. So the measured atomic mass is the mass of the sample Divided by the moles, which is equal to 63.67 g per mole. So therefore the atomic mass of the sample is 63.67 g per mole

Corporate society composite. I see you just to thus s afford double minus. So there are two electrons. Bar copper Adam. So well, number off copper Adams is given by go to the shark so divided by two it was guard into might start by time. Divided by do it was one amp times 3602nd, divided by to we have divided by the charge of the electron as well. 14 in six times, 10 to the negative. 19. Good. Um so that comes out as 1.1 to 5 stamps tended at 22 Adams, Mass. Off one copper atom in that case would be given by 1.185 Graham, divided by 1.125 times 10 to the 20 do equals 1.5 times 10 to the negative. 22 g. No, that finally, the mother mass off corporate will come out to be Alberta's number much diet by mass. Off one cooperative Adam equals 6.0 to 3 times 10 to the 23 times 1.5 times 10 to the negative. 22 equals 63.4 Grandpa. More


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