The people of pharmaceutical manufacturing is an expensive one. Many kind of drugs have actually several procedures in their synthesis and usage costly steustatiushistory.orgicals. A good deal of study takes place to build better methods to make drugs quicker and also more properly. Studying just how much of a compound is developed in any provided reaction is a crucial component of cost control.

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Percent Yield

steustatiushistory.orgical reactions in the actual human being don"t constantly go precisely as planned on paper. In the course of an experiment, many points will certainly add to the development of much less product thanpredicted. Besides spills and other speculative errors, there are commonly losses as a result of an incomplete reactivity, unpreferable side reactions, and so on steustatiushistory.orgists need a measurement that indicates just how successful a reactivity has been. This measurement is dubbed the percent yield.

To compute the percent yield, it is first crucial to recognize exactly how much of the product need to be developed based upon stoichiometry. This is referred to as the theoretical yield, the maximum amount of product that deserve to be developed from the provided quantities of reactants. The actual yield is the amount of product that is actually formed as soon as the reaction is lugged out in the laboratory. The percent yield is the ratio of the actual yield to the theoretical yield, expressed as a portion.

< extPercent Yield = frac extActual Yield extTheoretical Yield imes 100\%>

Percent yield is incredibly crucial in the manufacture of products. Much time and also money is spent improving the percent yield for steustatiushistory.orgical manufacturing. When complicated steustatiushistory.orgicals are synthesized by many various reactions, one step via a low percent yield can easily cause a big waste of reactants and also unnecessary price.

Generally, percent yields are understandably much less than (100\%) bereason of the reasons indicated earlier. However, percent returns higher than (100\%) are possible if the measured product of the reactivity has impurities that reason its mass to be greater than it actually would be if the product was pure. When a steustatiushistory.orgist synthesizes a desired steustatiushistory.orgical, he or she is always mindful to purify the commodities of the reaction. Example (PageIndex1) illustprices the actions for determining percent yield.

Example (PageIndex1): Decomposition of Potassium Chlorate

Potassium chloprice decomposes upon slight heating in the existence of a catalyst, according to the reaction below:

<2 ceKClO_3 left( s ight) ightarrow 2 ceKCl left( s ight) + 3 ceO_2 left( g ight) onumber>

In a details experiment, (40.0 : extg : ceKClO_3) is heated until it entirely decomposes. The experiment is percreated and the oxygen gas is accumulated and its mass is found to be (14.9 : extg).

What is the theoretical yield of oxygen gas? What is the percent yield for the reaction?


a. Calculation of theoretical yield

First, we will certainly calculate the theoretical yield based on the stoichiomeattempt.

Tip 1: Identify the "given" indevelopment and what the trouble is asking you to "find".

Given: Mass of (ceKClO_3 = 40.0 : extg)

Mass of O2 accumulated = 14.9g

Find: Theoretical yield, g O2

Step 2: List various other known amounts and also arrangement the difficulty.

1 mol KClO3 = 122.55 g/mol

1 mol O2 - 32.00 g/mol

Step 3: Apply stoichiomeattempt to transform from the mass of a reactant to the mass of a product:


Given: 1.274 g CuSO4

Actual yield = 0.392 g Cu

Find: Percent yield

List various other known amounts.

1 mol CuSO4= 159.62 g/mol 1 mol Cu = 63.55 g/mol

Since the amount of product in grams is not compelled, just the molar mass of the reactants is needed.

Balance the equation.

The steustatiushistory.orgical equation is currently balanced.

The well balanced equation offers the connection of 1 mol CuSO4 to 1 mol Zn to 1 mol Cu to 1 mol ZnSO4.

Prepare a idea map and also use the correct convariation variable.


The gave information identifies copper sulfate as the limiting reactant, and so the theoretical yield (g Cu) is discovered by performing mass-mass calculation based upon the initial amount of CuSO4.

Cancel units and also calculate.

Using this theoretical yield and also the provided value for actual yield, the percent yield is calculated to be:

Think about your outcome. Because the actual yield is slightly much less than the theoretical yield, the percent yield is just under (100\%).

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Theoretical yield is calculated based upon the stoichiometry of the steustatiushistory.orgical equation. The actual yield is experimentally identified. The percent yield is figured out by calculating the ratio of actual yield to theoretical yield.