Density & Moles!

The formula for Density is:
d=m/v

The conversion between Density and Moles is a two step process.

Example:
How many moles are in a 25.0mL sample of Iron if the density of Iron is 7.87g/mL

Step 1: Convert from Density to Mass using the equation.
25.0mL x 7.87g/1mL = 197g

Step 2: Convert from Mass to Moles using Molar Mass
197g x 1mol/55.8g = 3.53mol

Lab 4B from Heath Chemistry Lab Manuel

In class, our the purpose of our Lab was: To find out how many moles, raio of atoms of formula units are produced in the reaction of iron and copper (II) chloride.

Materials: Beaker, Washbottle, Stirring Rod, Tongs, Scapula, Scale, Drying oven, Safety goggles, Filter, Copper (II) Chloride, 2 Iron nails, 50 mL of distilled water

Procedure:
1. Find the mass of a dry 250 mL beaker, the 2 nails, and the piece of paper you are using to place the copper (II) chloride. Record it's mass using the scale.
2. Add the chloride onto the paper until you have reached 7 grams (Make sure it's below 10g)
3. Add the powder into the beaker
4. Weigh the beaker with the Copper (II) Chloride powder and record it's mass.
5. Add 50 mL of distilled water into the beaker filled with the powder. NOTE: To prevent spillage, use a stirring rod.
6. Add the 2 nails into the beaker filled with the solution.
7. Wait 10-15 minutes.
8. Remove the nails from the beaker one by one, with tongs.
9. Holding the nails above the beaker, spray them with water to remove the copper. NOTE: The less water sprayed, the less water to filter.
10. Once the copper is removed from the nails, set them to dry.
11. As the nails are drying, filter the Copper by decanting.
12. Take the filtered paper filled with copper and set it into the drying oven to dry.
13. After both the nails and filter paper of copper are dry, measure their masses.
14. Clean up all lab stations and equipment.