## What Percent Yield Calculator calculator does?

Are you frustrated with handling too many chemistry problems at once? Working on your product forecasting assignment to figure out whether the factory can really produce the 1000 units you just sold? If you need to manage actual yield vs. theoretical yield for a procedure, you are at the right place.

This user friendly percent yield calculator is designed in a way that if you can provide us with two of three values, we'll calculate the third missing value for you.

Following operations can be performed:

- The
**Percent Production**for the Experiment. - Provided with values of
**Theoretical Yield**and**Percentage Output**? We Foretell**Actual Yield.** **Provided with values of****Actual and****Percent Yield**? We Foretell**Theoretical output**

## Percent Yield and Its Significance

It is described as the proportion of the real to theoretical production. It explains the efficacy of a chemical reaction and is considered in different experiments like the simple decomposition of a compound.

In a nutshell, the percent yield calculator tells you the accuracy of your experiment. Let’s suppose an ideal condition, where you were very cautious with your reaction, made sure that the reaction was perfect, without accidents, your proportional yield would be 100%.

Above mentioned situation is idealized, it’s practically impossible to have 100% yield, If 100% it means you still have solvents or some contaminants in your end product. The proportional output will be less than 100% because of the difference between the actual and theoretical production.

Percent yield is quite significant in manufacturing different products. Let’s consider the process for making a drug called “Aspirin”. It has only a yield of 1%, it means the process is inefficient.

Carrying on with such low yield means wasting time and resources. So in this way, it helps the industries produce an optimum product with least waste.

## Actual vs. Theoretical yield:

The actual yield is the quantity of the end product in a chemical reaction. In comparison, the theoretical yield is the amount of product acquired through complete conversion of all the reactants into the final product, without any loss of reactant.

Generally, the actual yield is less than the theoretical yield because only few reactions actually advance towards completion. Some part of the product is not recovered at the end of the reaction. For instance, if you are recovering some precipitate of a product, you may lose other parts of it because of improper filtration. During the filtration process, some part of the product may not be sieved and left on the mesh paper.

## Percent Yield Formula:

In this formula, the proportion is computed by means of the **actual yield** of your product (i.e., amount of product made) and **the theoretical yield** of the product (i.e., the ideal mass if all molecules were consumed, none was lost). The formula is:

Percent yield = (Actual mass of desired product / Theoretical mass) ×100

The estimation requires you to provide two of the three variables, but it doesn't matter which two! Like any other equation, it can be readjusted to find the required variable. Don’t worry, this is made easy with the use of our smart calculator; just enter the two known variables to find the unknown within a fraction

## Calculation:

As you may have deduced from the equation above, if you want to determine the yield, you require two things, the actual and theoretical output.

You will need to find the moles or concentration in grams of your reactants to find the theoretical yield. Make sure you convert the concentration to a single unit: either grams or moles. Let's consider you have both the values; how will you find the output?

- Know the weights of both values (same units)
- Divide the actual yield with the theoretical one.
- Now, multiply this value by 100 to get the answer.

That’s it, not too complex right! Or you could **benefit from our smart percent yield calculator to find it easily and quickly.**

An important point about the values obtained; it’s possible to have a value above 100% but is due to the presence of solvent in your sample as well as in your end product. One solution is thorough drying of the product then reweigh it to get the true value. The right requirement is somewhere in 70-90% or more but never 100%.

## An example:

Let’s assume that you are conducting a nucleophilic addition reaction, using acetone and sodium cyanide to produce hydroxyacetonitrile.

For now, just ignore the solvents below the arrow; you reacted 7 g of acetone with 3 g of cyanide, giving a hypothetical production of 8.54 g of hydroxylacetonitrile. Now if you carry out the experiment and get actual yield of 7.58 g of hydroxylactenitrile, what will be the percent yield?

- You have the required values as the actual yield is 7.58 g, and theoretical yield is 8.54 g. Now use the following equation :

Percent yield = (Actual mass of desired product / Hypothetical mass) ×100

= (7.58 / 8.54)×100 = 88.75%

There it is: 88.75%. That was quite efficacious reaction! That will boost your confidence regarding the manufacturing process of the product. If you get a low output, don’t be upset, just repeat the experiment and this time try not to lose any of your reaction mixture.

Sometimes you may get more than 100%. It means you need to dry your product further then reweigh it and determine the production. It will come down to acceptable levels. Now that you have the basic concepts of the whole process, you can get maximum benefit from our smart tool.