EMPIRICAL FORMULA CALCULATION FROM LAB DATA
1. In an experiment similar to the zinc chloride experiment, a student placed a piece of lead in
hydrochloric acid. Hydrogen gas was given off, then the liquid was evaporated off. The remaining
solid, lead chloride, was massed. Use the data below to determine the empirical formula of lead
chloride. REMEMBER THE PROCEDURE FROM YOUR LAB.
mass of beaker
mass of lead and beaker before reaction
mass of lead chloride and beaker after reaction
mass of lead used in reaction
mass of lead chloride produced
mass of chlorine used in reaction
204.35 g
214.71 g
218.26 g
WORK:(show all work with units and appropriate sig figs)
a. Calculate the mass and moles of Pb that was used in the reaction.
(10.36g, 0.0500mol Pb)
b. Calculate the mass of lead chloride that was produced in the reaction.
(13.91g)
c. Calculate the mass and moles of chlorine that is in the lead chloride (HINT: subtract out the Pb)
(3.55 g, 0.10mol Cl)
d. Calculate the mol ratio of mol Cl/mol Pb
e. Write the empirical formula (the lowest ratio of subscripts) of lead chloride:
(2/1)
(PbCl2)
2. Below are the lab results of a reaction producing an iron chloride compound. Using the same process as in
your Empirical Formula Lab, calculate the empirical formula of the iron chloride compound (FexCly).
mass of beaker
mass of iron and beaker before reaction
mass of iron chloride and beaker after reaction
mass of iron used in reaction
mass of iron chloride produced
mass of chlorine used in reaction
63.12 g
65.73 g
70.67 g
WORK:(show all work with units and appropriate sig figs)
a. Calculate the mass and moles of Fe that was used in the reaction.
b. Calculate the mass of iron chloride that was produced in the reaction.
c. Calculate the mass and moles of chlorine that is in the lead chloride (HINT: subtract out the Fe)
d. Calculate the mol ratio of mol Cl/mol Fe
e. Write the empirical formula (the lowest ratio of subscripts) of iron chloride: