Here is the full lab:
Lab: Electrolytic Cells
Purpose: The purpose of this experiment is to test the method 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.
I get 117.34 grams
Place the steel can in the large beaker.
Pour the solution of tin(II) chloride into the beaker so it surrounds (but does not go in) the steel can.
Place the tin electrode into the beaker.
Attach the wires to the steel can and the tin electrode.
Connect the wires to the proper terminus on the power source.
Set the timer to 6.00 minutes and start the timer.
The power source will come on automatically and will turn off automatically when time runs out.
Take the mass of the steel can.Assume it is completly dry when you do so.
I get 118.05 grams
Analysis:
What is the mass of the tin produced?
Thank you
The mass of the Sn produced is the difference between the starting mass of the steel can before the procedure started and the mass of the steel can after the experiment was completed. What is that? About 118.05 - 117.34 = ??
Thank you
The mass of the tin produced is 0.71 grams
What is the theoretical mass of tin that should have been produced?
I have worked this problem several times over the last three-four days. You would do well to post ALL of your questions that deal with the experiment ALONG WITH YOUR WORK TO SHOW WHAT YOU HAVE DONE, explaining as you go what steps you don't understand and WHY you don't know the next step to take. Doing it this way you can drag it out for several days AND we will have done all the work for you, bit by bit. Done all together, you may understand how the problem works.
To find the mass of the tin produced in this electrolytic cell experiment, we need to use the principles of stoichiometry.
Stoichiometry is a branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. In this case, the tin(II) chloride solution is being electrolyzed to produce tin metal.
The balanced chemical equation for the reaction can be written as follows:
SnCl2(aq) → Sn(s) + 2Cl-(aq)
From the equation, we can see that for every one mole of tin(II) chloride reacted, one mole of tin is produced.
To find the number of moles of tin produced, we need to calculate the change in mass of the steel can before and after the experiment.
Initial mass of the can = 117.34 g
Final mass of the can = 118.05 g
Change in mass = Final mass - Initial mass
Change in mass = 118.05 g - 117.34 g
Change in mass = 0.71 g
Now, we need to convert the change in mass of the can to moles of tin.
The molar mass of tin (Sn) is approximately 118.71 g/mol.
Moles of tin = Change in mass / Molar mass
Moles of tin = 0.71 g / 118.71 g/mol
Moles of tin ≈ 0.00598 mol
Therefore, the mass of tin produced in this experiment is approximately 0.00598 moles.