hey drbob222

do you think you could help me out with this 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:
1. Take the mass of the steel can and record your observations.
2. Place the steel can in the large beaker.
3. Pour the solution of tin (II) chloride into the beaker so it surrounds (but does not go into) the steel can.
4. Place the tin electrode into the beaker.
5. Attach the wires to the steel can and the tin electrode.
6. Connect the wires to the proper terminus on the power source.
7. 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.
8. Take the mass of the steel can. Assume it is completely dry when you do so.

Analysis:
1. What is the mass of the tin produced? Show all your work.
2. What is the theoretical mass of tin that should have been produced? Show all your work.
3. Determine the accuracy of your result, using a percentage difference and discuss any discrepancies. Show all your work.

You didn't post anything.

Sure, I'd be happy to help you with your lab on Electrolytic Cells! Let's go through the procedure and then I'll explain how to answer each question in the analysis section.

Procedure:
1. Take the mass of the steel can and record your observations.
2. Place the steel can in the large beaker.
3. Pour the solution of tin (II) chloride into the beaker so it surrounds (but does not go into) the steel can.
4. Place the tin electrode into the beaker.
5. Attach the wires to the steel can and the tin electrode.
6. Connect the wires to the proper terminus on the power source.
7. 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.
8. Take the mass of the steel can. Assume it is completely dry when you do so.

Now let's move on to the analysis questions:

1. What is the mass of the tin produced? Show all your work.
To determine the mass of the tin produced, you need to find the difference in mass of the steel can before and after the experiment. Subtract the mass of the steel can before the experiment from the mass of the steel can after the experiment. This gives you the mass of the tin produced.

2. What is the theoretical mass of tin that should have been produced? Show all your work.
To find the theoretical mass of tin that should have been produced, you need to use stoichiometry. Start by balancing the chemical equation for the reaction between tin (II) chloride and the tin electrode. From the balanced equation, determine the mole ratio between tin (II) chloride and tin. Then, using the molarity of the tin (II) chloride solution, calculate the moles of tin (II) chloride used in the reaction. Finally, convert the moles of tin (II) chloride to the mass of tin using the molar mass of tin. This will give you the theoretical mass of tin that should have been produced.

3. Determine the accuracy of your result, using a percentage difference and discuss any discrepancies. Show all your work.
To determine the accuracy of your result, you need to calculate the percentage difference between the mass of tin actually produced (from question 1) and the theoretical mass of tin (from question 2). Use the following formula:
Percentage Difference = |(Actual Mass - Theoretical Mass) / Theoretical Mass| * 100%

If the percentage difference is close to 0%, it means the experimental result is very close to the theoretical value. If there is a significant percentage difference, it indicates some discrepancies between the experimental procedure and theoretical expectations.