Question

What mass of silver would be deposited if a 6.5 A current is passed through an aqueous solution of silver nitrate for 8.0 minutes?

Answer 1

@PANTIEPOWER

Answer 2

0.0 dunno know lol sorry @abb0t Mr. king

Answer 3

@abb0t anything?

Answer 4

Well, FIRST, you need to set up your \(\sf \color{red}{balanced~ chemical ~equation}\).
Then, you need to find the amount of moles, divide by faradays constant. which is \(\sf 9.65 \times 10^4 ~\frac{C}{mol}\)
Then multiply, which eliminates the Ampere units giving you moles of electron.

Answer 5

You need to get it in seconds also, by the way.

Answer 6

convert 8.0 mins \(\sf \rightarrow\) seconds

Then, once you have your moles of electron, use dimensional analysis to find your moles of silver.

Answer 7

I'm really confused haha @abb0t

Answer 8

let's go step by step, start by writing down the balanced chemical equation, can you do that?

Answer 9

Cu + AgNO3 --> CuNO3 + Ag ?

Answer 10

wait no Cu + 2AGNo3 --> Cu(No3)2 + 2AG

Answer 11

@abb0t @aaronq

Answer 12

Good, now convert minutes to seconds and divide! This will give you coulombs, which you can then use to divide by \(faraday's~constant\), which i posted up above, the 96500..

Answer 13

This will give you moles.
Then, using your balanced chemical equation, convert from what you have to what you want. Do you follow me still?

Answer 14

so 8 mins = 480 seconds but what am I dividing?

Answer 15

@abb0t

Answer 16

Follow the units, it will tell you what you need to divide by.

Answer 17

I believe it should be Ampere per seconds.

Answer 18

so 6.5/480 = 0.013542
then that divided by F constant is 1.40331606e-7
what next?

Answer 19

@abb0t

Answer 20

@Abmon98 ?

Answer 21

yes.

Answer 22

what's next? @abb0t

Answer 23

Did you divide by faradays constant?

Answer 24

yes

Answer 25

notice that you are left with moles.

Answer 26

1.40331606e-7 moles?

Answer 27

No, not that one. I already provded it for you up above!

Answer 28

I'm so sorry I'm so lost hahaha @abb0t

Answer 29

Look up above. 96500...

Answer 30

right the 9.65×10^4

Answer 31

I divided 6.5/480 = 0.013542 and then I divided that by faraday and i got 1.40331606e-7

Answer 32

\(\large{\frac{0.013542}{96500}}\) = mol \(\sf \times \frac{mol~want}{mol~have}\)

Answer 33

This is where you will utilize your balanced chemical equation to convert! Do you follow me?

Answer 34

ok yes I follow you now

Answer 35

Now that you have your moles, convert to moles of Ag, since you have Ag(NO3), note that it is a 2:2 ratio (i think if you wrote it correctly - make sure it is).
so you have \(\sf \frac{2~mol~ Ag}{2~mol~Ag(NO3)}\) = mol Ag
now, you can use molar mass to convert and find the mass. Remember that molar mass is grams per mol, so make sure that you look at your periodic table, and look for Ag - silver.

Answer 36

so \[\frac{ 0.013542 }{ 96500 } = mol Ag\]

and then

\[1.40331606\times10^{-7} \times 107.86820\]

Answer 37

@abb0t

Answer 38

I got a wrong answer... hmm I got 0.00001513731 but the answer choices are as follows:

Answer 39

I got one of those answers.

Answer 40

\(\large{\frac{6.5 \times 480~s}{96500 }}\) = __________ mol

your mole is incorrect. I don't know where you're getting such a low mole value!

Answer 41

check your math again.

Answer 42

You should get 3.459...

Answer 43

@abb0t this helped me a lot