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 got 117.34 grams

2Place the steel can in the large beaker.
Pour the solution of tin (II) chloride into the beaker so it surrounds (but does not go into) 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 completely dry when you do so.

I got 118.05 grams

Analysis:
What is the mass of the tin produced? Show all your work.

Thank you

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? Show all your work.

Thank you

CuNo3+AlOH blace

To calculate the mass of tin produced, we need to use stoichiometry and the balanced equation for the reaction happening in the electrolytic cell. The balanced equation for the reaction is as follows:

Sn^2+ (aq) + 2e^- → Sn (s)

From the equation, we can see that for every 2 moles of electrons (2e^-), we get 1 mole of tin (Sn). Now, let's calculate the number of moles of tin produced using the information given.

1. Convert the mass of the steel can to moles:
The molar mass of tin (Sn) is 118.71 g/mol.
Therefore, the number of moles of steel can = (118.05 g - 117.34 g) / 118.71 g/mol.

2. Calculate moles of electrons:
Using Faraday's law, we know that 1 mole of electrons is equal to 96485 C (Coulombs).

3. Calculate the number of moles of tin:
According to the balanced equation, the ratio of moles of electrons to moles of tin is 2:1. Therefore, the number of moles of tin produced is equal to half the moles of electrons.

4. Finally, calculate the mass of tin produced:
Mass of tin = moles of tin * molar mass of tin.

Following these steps, you can calculate the mass of the tin produced in this electrolytic cell experiment.