LAB: Iron and and Copper Chloride

Problem: What is the ratio of moles of Copper formed to moles of Iron reacted in the chemical reaction described below?

To find the answer to this question our group placed an Iron nail in a solution of Cupric Chloride after measuring the filter paper and mass of the nail. We observed an immediate change in the color of the nail; it turned a rusty red. We learned that the iron was dissolving. These dissolved iron particles will combine to form Ferric Chloride. After, we removed the nail form the solution and dried it then we transfered the solution in to a separate beaker using filter paper. We measured the mass of the nail. It took a long time for the solution to filter. We determined the mass of Iron consumed  by comparing the mass of the nail before and after the reaction. After the solution had filtered we transferred the Ferric Chloride and the filter paper to dry in the drying oven. We have yet to measure its mass then we can determine the mass mass of the Ferric Chloride formed.

Group: Jennifer, Jomar, Paulette

Density and Moles

Density
-Density is a measure of mass per volume d = m
                                                                      V
-measured in g/L or g/mL

Example
-Water has a density of 1.0g/mL. Determine the mass of 11.5mL of water
-How many moles are in 11.5mL of water?

1.0g/mL x 11.5mL = 11.5g
11.5g x 1 mol = 0.64 mol
             18 g

Density of Gases

-The density of gases varies with temperature

-At STP we can find density by:  MM              molar mass               

                                               22.4L/mol        molar volume

Example
-Calculate the density of 02 STP

32.0g/mol = 1.43g/L
22.4L/mol

-An unknown diatomic gas has a density of 1.696g/mol STP
 -Find its molar mass
 -What is the chemical formula

1.696g/L x 22.4L/ 1 mol = 37.99g/mol = 38g/mol
                                                                  2
                                                            = 19g/mol
Chemical formula : F2