# Percent Yield Calculator

Our percent yield calculator will help you to understand **how to calculate percent yield**, as well as teach you the **percent yield formula and the percent yield definition**. Finding the yield is an integral part of any kind of synthetic lab work as **the percent yield equation turns your experimental yields into a representation of how successfully you carried out your reaction**. Hopefully, after reading this page, you will have an answer to the questions "how to find percent yield?" and "what is percent yield?"

## Percent yield definition

What is percent yield? The percent yield definition is that it is a measure of the effectiveness of a synthetic procedure. Wordy, right? To put it simply, **percent yield tells you how well you carried out your reaction**. If you were very careful with your reaction, made sure every molecule reacted and that nothing was lost when you poured the solution from one beaker to another, your percent yield would be $100\%$ (don't worry if you don't get $100\%$, this is practically impossible). If you accidentally poured your reaction mixture down the drain and lost everything, then your percent yield would be $0\%$, and if you still had a lot your solvent present with the product, your yield would be greater than $100\%$. **Still confused how to find the percent yield? Check the percent yield equation below!**

A percent yield of $100\%$ corresponds to the theoretical yield: discover this quantity with the theoretical yield calculator.

## Percent yield formula

The percent yield can be found using the percent yield equation. It is expressed a simple percentage calculated by **using the experimental yield** (we learned how to calculate it with our actual yield calculator) of your product (i.e., how much of your product you made) **and the theoretical mass** of the product (i.e., the mass if not a single molecule was lost). The percent yield formula is:

Where:

- $Y_{\text{p}}$ — The percent yield;
- $m_{\text{p},\text{exp}}$ — The experimental mass of the product; and
- $m_{\text{p},\text{th}}$ — The theoretical mass of the product.

The percent yield equation requires you to know two of the three variables, but it doesn't matter which two! Like any equation, it can be rearranged to find the unknown, but there's no need to worry about this when you can use our smart calculator; just enter the two known variables and find the third.

## How to calculate percent yield

As you may have guessed from the percent yield equation above, if you want to know how to calculate the percent yield, you need two things, your experimental yield and the theoretical yield. Let's assume you have both values; how to find the percent yield?

🙋 You may need to find the mole or concentration of your reactants to find the theoretical yield: use our tools, the mole calculator and the concentration calculator.

- First make sure the both weights have the same units (use our weight converter if you need some help 😉).
- Take your experimental yield and divide it by the theoretical yield.
- Multiply this value by $100$ to find the percent yield.

There you go, not too complicated right! Or you could **use our percent yield calculator to calculate it easily and quickly**. A note about the values obtained; a value above $100\%$ is possible but is due to solvent being present in the sample as well as your product. Dry your product thoroughly and re-weight to get the true percent yield. Also, a value of 100% is impossible to achieve; there will always be some molecules that do not react or that are left on the side of the glassware. A value of $70\%$ or higher is acceptable!

## Examples of yield calculations

Time for some examples. Lets say you are doing a nucleophilic addition reaction, forming hydroxyacetonitrile from sodium cyanide and acetone.

Let's ignore the solvents underneath the arrow; we reacted $5\ \text{g}$ of acetone with $2\ \text{g}$ of cyanide, giving a theoretical yield of $6.54\ \text{g}$ of hydroxyacetonitrile. Now we know that if we carry out the experiment and get $5.58\ \text{g}$ of hydroxyactenitrile, what is the percent yield?

- We know our experimental yield is $5.58\ \text{g}$, and our theoretical yield is $6.54\ \text{g}$. Let's use the percent yield formula from above: $Y_{\text{p}} =m_{\text{p},\text{exp}}/m_{\text{p},\text{th}}\cdot 100$ and fill in the fields:

The percent yield is $85.3\%$. That was a pretty successful reaction! You should feel a bit more confident at knowing how to calculate theoretical yield now. Let's try another example to bolster that confidence.

You react $8\ \text{g}$ of calcium carbonate with $9\ \text{g}$ of acetic acid, forming $4.35\ \text{g}$ of acetone. Nice! Now we do this reaction, but, unfortunately, we only get $1\ \text{g}$ of acetone. What is the percent yield?

- Our experimental yield is $1\ \text{g}$, and our theoretical yield is $4.35\ \text{g}$. Using the percent yield formula again gives us:

Now that's not great. Don't be upset though, there's plenty of time left in the lab session, so you try again. This time you try really, really hard to not lose any of your reaction mixture, and you end up with a yield of $5.31\ \text{g}$. Well, that's much better than last time, so you carry out a percent yield calculation:

Oh no! The percent yield is over $100\%$, meaning that there is still some solvent in our product. This means we need to dry our product further, so let's do that. After re-weighing our product (this time with no solvent) we find it has a weight of $4\ \text{g}$. Let's calculate the percent yield:

Fantastic! Now you should have a grasp on the basics of percent yield calculation, and with it have the knowledge you need to make the most out of our website. Happy calculating!