Stoichiometry to Determine Percent Yield (Lab Report Sample)

Name
Professor’s name
Subject
Date
Stoichiometry to Determine Percent Yield
Abstract
The stoichiometry of a chemical reaction is the arithmetic relationship between the products moles and the reactants moles for the reaction. The experiment is intended to delineate the relationship between amounts of reactants and the products amount resulting from a chemical reaction. The standards of limiting reagent and stoichiometry will be utilized to foresee the measure of the item that ought to be created when blending two solutions for insoluble product production.
The percentage yield is sometimes obtained may be more than 100 % due to measuring mistakes, or extra substance present in the product making it weigh more than expected. The objective of this experiment is to determine the percentage yield of calcium chloride when Calcium carbonate react with sodium chloride.
Introduction
The stoichiometry of a chemical reaction is the arithmetic relationship between the products moles and the reactants moles for the reaction. On the other hand, limiting reagent is the reactant that get consumed completely in a chemical reaction.
This experiment is intended to delineate the relationship between amounts of reactants and the products amount resulting from a chemical reaction. The standards of limiting reagent and stoichiometry will be utilized to foresee the measure of the product that ought to be created when blending two solutions for insoluble product production.
The reaction is as follows;
Ca Cl2(aq)+NaCO3(aq) →2NaCl(aq)+CaCO3(s)
Ionic equation for above chemical reaction is as follow;
Ca2+ (aq) + CO3-(aq) → CaCO3(s)
Since calcium chloride contains one mole of Ca2+ per mole of CaCl2 and sodium carbonate contains one mole of the CO3-per mole of NaCo3, the reagent with the least number of moles will be restricting. Hypothetically, for each mole of limiting reagent, a mole of Calcium Carbonate, ought to be framed because there is a 1:1 mole proportion of both reactants as show in above balanced chemical equation. Multiplying this theoretical yield by the molar mass of CaCO3 leads to the yield in grams.
The experiment finds the percent yield calculated by determining ratio of the actual yield (in grams) to theoretical yield (grams) as follows;
% yield=actual yield (grams)Theoretical yeild (grams)*100%
Methods
Four beakers to hold reaction mixtures were labeled while using Erlenmeyer flask two stock of solution were obtained and their concentration recorded. Burette was filled with calcium chloride solution after rinsing. Initial burette reading were also on the data sheet.
Burette was also filled with sodium carbonate solution after rinsing and their values recorded in the data sheet. The reaction flask was filled with the solution as provided (Table 1) with volume registered in the data sheet.
Table 1. Volume of calcium chloride and sodium carbonate used.

CaCl2(Ml)

Na2 CO3 (Ml)

Reaction 1

25

25

Reaction 2

28

25

Reaction 3

10

25

Reaction 4

25

10

Each reaction was stirred with stirring rod and then transferred to another beaker. For each reaction, the following were done;
The filter paper was pre-weighted on a watch glass using analytical balance. The content of the beaker were filtered, using the filter paper, and its contents were transferred to watch glass, then dried under the heat lamp. The contents of watch glass were weighed after drying and all the masses recorded in the data sheet.
Data
Table 2. Volume of Calcium chloride

Trial #1

Trial #2

Trial #3

Trial #4

Concentration(M)

0.05

0.05

0.05

0.05

Initial reading (ml)

0.00

0.00

28.10

5.00

Final reading (ml)

25.00

28.10

38.10

30.00

Volume delivered(ml)

25.00

28.10

10.00

25.00

Table 3. Volume of sodium carbonate

Trial #1

Trial #2

Trial #3

Trial #4

Concentration(M)

0.05

0.05

0.05

0.05

Initial reading (ml)

0.00

25.00

0.10

25.10

Final reading (ml)

25.00

50.00

25.00

35.00

Volume delivered(ml)

25.00

25.00

25.00

10.00

Table 4; Mass of product

Trial #1

Trial #2

Trial #3

Trial #4

Watch glass + filter paper

36.2036

54.8157

49.6542

49.5005

Watch glass+ filter p + product

36.2902

54.9125

49.9090

49.5852

Mass of the product

0.0864

0.0968

0.0548

0.0847

Table 5, summary of above tables (2-4)

Trial #1

Trial #2

Trial #3

Trial #4

Volume of Calcium Chloride (ml)

25.00

28.00

10.00

25.00

Volume of sodium carbonate (ml)

25.00

25.00

25.00

10.00

Mass of the product (g)

0.0864

0.0968

0.0548

0.0847

Calculation
Table 6. Theoretical number of moles

Trial #1

Trial #2

Trial #3

Trial #4

No. of liters of sodium Carbonate used.

0.00025

0.00025

0.00025

0.001

No. of liters of calcium chloride

0.00125

0.0014

0.0005

0.00125

Limit reagent

CaCl2

CaCl2

CaCl2