# Lab 3 Requirements

Topics: Stoichiometry, Yield, Mole Pages: 1 (280 words) Published: February 18, 2013
This document is not meant to be a substitute for a formal laboratory report. The Lab Report Assistant is simply a summary of the experiment’s questions, diagrams if needed, and data tables that should be addressed in a formal lab report. The intent is to facilitate students’ writing of lab reports by providing this information in an editable file which can be sent to an instructor. Observations

When using 1.0 g of CaCl2·2H2O, stoichiometric calculations should give the following results: 1 g CaCl2·2H2O x 1 mole CaCl2·2H2O x 1 mol Na2C03 x 106 g Na2C03 = 147 g CaCl2·2H2O 1 mol CaCl2·2H2O 1 mol Na2C03

Using 1 g of CaCl2·2H2O and .72 or .8 g (slight excess) Na2CO3 Should give a CaCO3 theoretical yield as follows:
1 g CaCl2·2H2O x 1 mole CaCl2·2H2O x 1 mol CaC03 x 100 g CaC03 = 147 g CaCl2·2H2O 1 mol CaCl2·2H2O 1 mol CaC03
To double-check, we can calculate CaCO3 theoretical yield by using Na2CO3 0.72 g Na2C03 x 1 mol Na2C03 x 1 mol CaC03 x 100 g CaC03 =
106 g Na2C03 1 mol Na2C03 1 mol CaC03
Experiment Stoichiometry of a Precipitation Reaction
Questions
A. From your balanced equation what is the theoretical yield of your product? B. According to your data table, what is the actual yield of the product? C. What is the percent yield?
D. A perfect percent yield would be 100%. Based on your results, comment on your degree of accuracy and suggest possible sources of error.
E. How could these errors be reduced in the future?