Stoichiometry Lab Report
Stoichiometry Lab Stoichiometry is the end result of adding up chemical elements that were involved in chemical reactions (http://dictionary.reference.com/browse/stoichiometry). The word stoichiometry was obtained from two greek words meaning element and measure. This explains the definition for the term. A chemist named Jeremias Benjamin Richter was the chemist responsible for first realizing what stoichiometry was (http://www.chemteam.info/Stoichiometry/What-is-Stoichiometry.html). In 1972, Jeremias published his theories about the law of definite proportions. Among this theory, he also discussed stoichiometry and what its role was used for when determining the weight of the chemical compounds of definite proportions. Richter showed a great interest towards the mathematical portion of chemistry, explaining how he was able to come up with the idea of stoichiometry (http://chemed.chem.purdue.edu/genchem/history/stoichiometry.html).
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The procedure for this lab are as follows below:
Part 1 of 2 NaHCO3 reacted with HCl:
The mass of the flask was recorded.
2.0 +/- 0.2 grams of NaHCO3 was added to the flask. The mass of NaHCO3 + flask was then recorded. Before moving on to step 3, the mass of NaHCO3 was calculated. Then the theoretical yield of NaCl was determined. This was the hypothesis.
30 mL of hydrochloric acid should be obtained.
HCl was slowly added to NaHCO3, drop by drop. The reactants should not splatter out of the flask.
When the liquid had begun to build up, the flask was gently swirled to further mix the reactants.
The acid was continuously added until the reaction was complete. The reaction was complete when the additions of HCl “bubbling” began to stop.
Part 2 of 2 The water is evaporated (heated to a constant
The procedure for this lab are as follows below:
Part 1 of 2 NaHCO3 reacted with HCl:
The mass of the flask was recorded.
2.0 +/- 0.2 grams of NaHCO3 was added to the flask. The mass of NaHCO3 + flask was then recorded. Before moving on to step 3, the mass of NaHCO3 was calculated. Then the theoretical yield of NaCl was determined. This was the hypothesis.
30 mL of hydrochloric acid should be obtained.
HCl was slowly added to NaHCO3, drop by drop. The reactants should not splatter out of the flask.
When the liquid had begun to build up, the flask was gently swirled to further mix the reactants.
The acid was continuously added until the reaction was complete. The reaction was complete when the additions of HCl “bubbling” began to stop.
Part 2 of 2 The water is evaporated (heated to a constant