TO DR.BOB222
hi i have a question. It's regarding a electrolytic cells. This lab has already been posted but i wanted to show you what i have so maybe you can check it for me.
question: what is the mass of tin produced?
what is the theoretical mass of tin that should have been produced?
Determine the accuracy of your results, using percentage difference and discuss any discrepancies?
question 1:
So my givens are:
Electrolyte: SnCl3
Current: 3.46A
Time: 6min (3600s)
step 1: Quantity of electricity in coulombs.
= 3.46A x 3600S
= =1245.6C
Step 2: Amount of electrons . 1 mole has a charge 96500C
amount of electrons= 1245.6 x 96500C
= 0.013mol e-
Step 3: Half reaction for reduction of tin
Sn^4+ + e- --> Sn^2+
amount of tin produced.
0.013mol e- x 1mol/4mol
= 0.00325mol of Sn
step 4:convert amount of tin to mass
mass formed= 0.00325mol sn x 118g
= 0.387g
I only read the first line or two, but isn't 6 min just 360 sec and not 3600?
6 min x (60 sec/min) = 360 seconds.
And are you sure the electrolyte is SnCl3 or is it SnCl2? And if you are plating out tin, wouldn't the half cell show Sn as the product instead of Sn^+2. Truthfully, I'm not familiar with your lab; however, check me out on the above.
yeah sorry about the 3600..in my lab i used 360 im not sure why i put 3600. And your right about the SnCl2 instead of SnCl3.
and as far as the half cell, since im using tin II chloride the half cell should be
Sn^2+ + 2e- --> Sn^+
Right?
this is the full lab..
purpose: to test the methos of stoichiometry in cells
materials:
balance
steel can
tin electrode
power source
wire lead (x2)
tin (II) chloride solution (3.25 M)
timer
large beaker
procedure
take the mass of the steel can and record your observations. 117.34g
place steel can into large beaker
place tin electrode into beaker
attach the wires to the steel can and the tin elextrode
connect the wires to the proper terminus on the power source
set timer to 6min and start timer
take the mass of the steel. 118.05g
questions
What is the mass of the tin produced? Show all your work.
What is the theoretical mass of tin that should have been produced? Show all your work.
Determine the accuracy of your result, using a percentage difference and discuss any discrepancies. Show all your work.
If you are plating out Sn, then the half cell must be Sn^+2 + 2e = Sn.
I'll look at the remainder but give me some time.
Changing the half reaction for Sn^+2 to Sn will change all of your other calculations but there are a couple of notes here.
1. I see you have used 96,500 C per Faraday but since your balance weighings were closer than that, I wonder why you haven't used 96,485? Of course, use 96,500 if those were your instructions.
2. When I divide 1245.6 by 96,500, I get 0.01291. You probably rounded up to 0.013 and your numbers should be better than that so I wouldn't round up. Of course, if you use 96,485, you still have 0.01291 as an answer.
3.I notice you used 118 for the atomic mass of Sn but on th table I have it is listed as 118.7.
well im not all that worried about rounding off my numbers. When it comes to actually handing in the assignment i use it the way it's given to me from the book. My question was if i am doing the equation correctly, and if you could help me get started with the following question, which was "what is the theoretical mass of tin that should have been produced?". What are the equations i use to get my answer?
All you need to do is to correct for the half cell reaction Sn^+2 + 2e ==> Sn.
Step 3: Half reaction for reduction of tin
Sn^4+ + e- --> Sn^2+
amount of tin produced.
0.013mol e- x 1mol/4mol
= 0.00325mol of Sn
This step then would be 0.0129 x 1 mol e/2 mol(instead of 4) = 0.00646 mols Sn
step 4:convert amount of tin to mass
mass formed= 0.00325mol Sn x 118g
= 0.387g
0.00646 mols Sn x (118.7 g Sn/1 mol Sn) = 0.766 g Sn. This is the theoretical yield.
You found 118.05 - 117.34 = 0.71 g Sn plated out in your experiment.
Percent error = [(correct value-your value)/correct value] * 100,
I get about 7 or 8% which isn't bad at all.
Hi there! I'd be happy to help you check your work on this lab question.
For question 1, you have correctly calculated the Quantity of Electricity (Q) in coulombs. This is determined by multiplying the current (A) by the time (s), giving you 1245.6 C.
In step 2, you correctly determined the amount of electrons produced. One mole of electrons has a charge of 96500 C, so you multiplied the Quantity of Electricity by this value to obtain 0.013 mol of electrons.
Next, in step 3, you correctly wrote the half reaction for the reduction of tin. The reaction shows that for every 1 electron used, 1/4 mole of Sn is produced. Since you have 0.013 mol of electrons, you can multiply this by the molar ratio (1 mol Sn/4 mol e-) to find the amount of tin produced: 0.013 mol e- x (1 mol Sn/4 mol e-) = 0.00325 mol Sn.
Finally, in step 4, you determined the mass of tin formed by multiplying the amount of tin produced (in moles) by the molar mass of tin (118 g/mol): 0.00325 mol Sn x 118 g/mol = 0.387 g.
Your calculation for the mass of tin produced looks correct based on the given information.
Now, let's move on to question 2, which asks for the theoretical mass of tin that should have been produced.
To calculate the theoretical mass of tin, we need to know the balanced chemical equation for the reaction and the stoichiometry of the reaction. Do you have this information? If not, please provide it so we can proceed with the calculation.
Once you have the balanced chemical equation and stoichiometry, you can follow a similar approach as in question 1 to calculate the theoretical mass of tin produced.
Let me know when you have the information for the balanced equation, and I'll help you proceed with the calculation.