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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.

To find the mass of the tin produced, we need to use stoichiometry. Stoichiometry is a method used to determine the quantities of reactants and products involved in a chemical reaction.

In this experiment, the tin(II) chloride solution is being electrolyzed, which means it is reacting to produce tin. The balanced chemical equation for this reaction is:

SnCl2(aq) → Sn(s) + 2 Cl- (aq)

From the equation, we can see that 1 mole of tin(II) chloride produces 1 mole of tin. Therefore, we need to convert the mass of the steel can into moles of tin, and then convert that into grams of tin.

First, find the change in mass of the steel can:

Change in Mass = Final Mass - Initial Mass
Change in Mass = 118.05 g - 117.34 g
Change in Mass = 0.71 g

Next, convert the change in mass of the steel can to moles of tin:

Molar Mass of Tin (Sn) = 118.71 g/mol (you can find this value on the periodic table)

Moles of Tin = Change in Mass / Molar Mass
Moles of Tin = 0.71 g / 118.71 g/mol
Moles of Tin ≈ 0.006 mol

Since the balanced equation tells us that 1 mole of tin(II) chloride produces 1 mole of tin, the moles of tin produced is also approximately 0.006 mol.

Finally, convert the moles of tin produced into grams of tin:

Molar Mass of Tin (Sn) = 118.71 g/mol

Mass of Tin = Moles of Tin × Molar Mass
Mass of Tin = 0.006 mol × 118.71 g/mol
Mass of Tin ≈ 0.71 g

Therefore, the mass of tin produced in this electrolytic cell is approximately 0.71 grams.