Copper Reactions
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ABSTRACT
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The copper reaction experiment was demonstrated by adding the reagents like 16M HNO3, Distilled water, 6M NaOH, 6M H2SO4, Acetone, Zinc metal and Methanol into the beaker with the copper wire. The experiment was also demonstrated to observe how copper reacts while different reagents were being added. It was also demonstrated to practice the common laboratory techniques such as methods of separation involving filtration, sedimentation, decantation and extraction. While different reagents were added to the copper wire, different reactions were also observed and tallied until the recovered copper was weighed and the percentage yield was calculated from the formula:
Percentage Yield=mass of recovered copperactual yieldmass of copper wire (theoretical yield) x 100
The percentage yield of the experiment was 42%.
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Introduction
All chemical reactions occurring within test tubes, industrial reactors, or nature, can be described by reaction equations. Knowing the skeletal reaction equation, the reactants and the products are also known, but for quantitative predictions, the reaction equation needs to be balanced.
A balanced equation is an equation or a chemical reaction in which the number of atoms for each element in the reaction and the total charge are the same for both the reactants and the products. (1) From a balanced equation, the mole relationship can be figured out. The amount of product produced from a given amount of reactants based on the balanced chemical equation is referred to as the theoretical yield. The theoretical yield is based on the stoichiometry of the reaction and ideal conditions in which starting material is consumed completely, undesired side reactions do not occur, and there are no losses in the work-up procedure. On the other hand, the
ABSTRACT
-------------------------------------------------
The copper reaction experiment was demonstrated by adding the reagents like 16M HNO3, Distilled water, 6M NaOH, 6M H2SO4, Acetone, Zinc metal and Methanol into the beaker with the copper wire. The experiment was also demonstrated to observe how copper reacts while different reagents were being added. It was also demonstrated to practice the common laboratory techniques such as methods of separation involving filtration, sedimentation, decantation and extraction. While different reagents were added to the copper wire, different reactions were also observed and tallied until the recovered copper was weighed and the percentage yield was calculated from the formula:
Percentage Yield=mass of recovered copperactual yieldmass of copper wire (theoretical yield) x 100
The percentage yield of the experiment was 42%.
____________________________________________________________
________________________
Introduction
All chemical reactions occurring within test tubes, industrial reactors, or nature, can be described by reaction equations. Knowing the skeletal reaction equation, the reactants and the products are also known, but for quantitative predictions, the reaction equation needs to be balanced.
A balanced equation is an equation or a chemical reaction in which the number of atoms for each element in the reaction and the total charge are the same for both the reactants and the products. (1) From a balanced equation, the mole relationship can be figured out. The amount of product produced from a given amount of reactants based on the balanced chemical equation is referred to as the theoretical yield. The theoretical yield is based on the stoichiometry of the reaction and ideal conditions in which starting material is consumed completely, undesired side reactions do not occur, and there are no losses in the work-up procedure. On the other hand, the
References: 1. Chemistry Glossary, Balanced Equation Definition., About.com. http://chemistry.about.com/od/chemistryglossary/a/balanceeqdef.htm 2. Vogel, A.I., Tatchell, A.R., Furnis, B.S., Hannaford, A.J. and P.W.G. Smith. Vogel 's Textbook of Practical OrganicHall, 19936-3. 3. A. Yaksic., Chemical Reactions of Copper and Percent Yield., Retrieved August 11, 2011. http://www.yaksic.com/crcpy6.pdf 4. Analytical Balance. (2011). In Encyclopædia Britannica. Retrieved from http://www.britannica.com/EBchecked/topic/22617/analytical-balance