Difference between revisions of "Percentage Yield"
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==Key Stage 3== | ==Key Stage 3== | ||
===Meaning=== | ===Meaning=== | ||
| − | The '''percentage yield''' is the | + | The '''percentage yield''' is the [[mass]] of a [[product]] in an [[Chemical Reaction|chemical reaction]] compared to the [[mass]] that could theoretically be produced in a perfect [[Chemical Reaction|reaction]] as a [[percentage]]. |
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| + | ===About Percentage Yield=== | ||
| + | : The '''percentage yield''' is useful to work out the efficiency of a [[Chemical Reaction|chemical reaction]] and considering the cost of forming the desired [[product]]. | ||
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| + | ===Equation=== | ||
| + | Percentage Yield = (Actual [[mass]] of [[product]]/Theoretical maximum [[mass]] of [[product]])x100% | ||
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| + | Percentage Yield = <math>\frac{M_A}{M_T}</math> | ||
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| + | Where: | ||
| + | : M<sub>A</sub> = Actual [[mass]] of [[product]] | ||
| + | : M<sub>T</sub> = Theoretical maximum [[mass]] of [[product]] | ||
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| + | ===Factors Affecting Percentage Yield=== | ||
| + | *[[Reversible Reaction]]s - Some [[Chemical Reaction|reaction]]s are [[Reversible Reaction|reversible]] which means the [[product]]s may [[Chemical Reaction|react]] to form the original [[reactant]]s resulting in less than 100% of the theoretical maximum [[mass]] of [[product]]. | ||
| + | *[[Pure|Purity]] of [[Reactant]]s - If the [[reactant]]s are not [[pure]] then there is not as much of the original [[chemical]]s as was believed, resulting in less [[product]] being formed. | ||
| + | *Collection of [[Product]] - Collecting and separating out the [[product]]s may not be an easy process and some of the [[product]] may be lost in the process. | ||
| + | *Unwanted [[Chemical Reaction|Reactions]] - Sometimes there may be other [[Chemical Reaction|chemical reaction]]s which take place in the [[Reaction Mixture|reaction mixture]], this may reduce the amount of desired [[product]]. | ||
Revision as of 11:29, 13 January 2019
Contents
Key Stage 3
Meaning
The percentage yield is the mass of a product in an chemical reaction compared to the mass that could theoretically be produced in a perfect reaction as a percentage.
About Percentage Yield
- The percentage yield is useful to work out the efficiency of a chemical reaction and considering the cost of forming the desired product.
Equation
Percentage Yield = (Actual mass of product/Theoretical maximum mass of product)x100%
Percentage Yield = \(\frac{M_A}{M_T}\)
Where:
Factors Affecting Percentage Yield
- Reversible Reactions - Some reactions are reversible which means the products may react to form the original reactants resulting in less than 100% of the theoretical maximum mass of product.
- Purity of Reactants - If the reactants are not pure then there is not as much of the original chemicals as was believed, resulting in less product being formed.
- Collection of Product - Collecting and separating out the products may not be an easy process and some of the product may be lost in the process.
- Unwanted Reactions - Sometimes there may be other chemical reactions which take place in the reaction mixture, this may reduce the amount of desired product.