An online innovative percent yield calculator helps you to calculate the percent yield value for a given amount of theoretical and actual yield. Our user-friendly yield percent calculator is the way to calculate the synthetic reaction that is done during lab experiments.

## Percent Yield Definition:

**Percent yield is the ratio between the mass of the actual yield and the amount of yield that we get after the completion of the chemical reaction.**

Percent yield calculator chemistry is used to determine the efficiency of a chemical reaction. Higher the yield more efficient the reaction, and vice versa.

## Percent Yield Formula:

The percent yield equation is determined by calculating the actual yield over the __theoretical yield__. The yield percentage calculator equation is:

**Percent Yield formula = mass actual yield/mass theoretical yield * 100%**

Yield is the total amount of product after a synthetic lab experiment. There are two components of yield.

## How To Calculate Percent Yield?

The percent yield calculator tells how well you carried out your reaction. But manual calculations are also very important. For this purpose, look at the example below:

### Example # 1:

Let's assume that you are conducting a nucleophilic addition reaction, using acetone (CH3)2CO and sodium cyanide (NaCN) to produce hydroxy acetonitrile.

For now, just ignore the solvents below the arrow; you reacted 7g of acetone with 3g of cyanide, giving a hypothetical production of 8.54g of hydroxyl acetonitrile.

Now, calculating percent yield if you carry out the experiment and get an actual yield of 7.58g of hydroxyl acetonitrile?

#### Solution:

Actual amount of product = 7.58 g

Expected amount of product = 8.54 g

Now use the following percent yield equation:

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

Percent Yield = (7.58 / 8.54)×100

= 88.75%

### Example # 2:

When 16.0 g of calcium carbonate (CaCO3) is heated to thermal decomposition, 7.54 g of calcium oxide (CaO) is obtained. How to calculate percent yield using the percentage yield formula?

**CaCO3 →CaO + CO2**

#### Solution:

Stoichiometry percent yield can be calculated by finding the percentages of the actual mass of the desired product to the hypothesis mass.

One mole of calcium carbonate gives one mole of calcium oxide.

The molar mass of calcium carbonate is 100 g/mol.

The molar mass of calcium oxide is 56 g/mol.

It means that if 100 g of CaCO3 was burnt, it gave 56 g of CaO. But in this experiment, 16 g of CaCO3 was burnt, then the amount of CaO should be:

Hypothesis Mass = 56 g / 100 g * 16 g

= 8.96 g

Now enter the actual yield and the expected amount of product means the hypothesis mass of chemical reaction to calculate the percent yield.

Percent yield formula = actual yield / theoretical yield * 100

Percent yield = 7.54 g / 8.96 g * 100

Percent yield = 84.16 %

## Working of Percent Yield Calculator:

Our percent yield of chemical reaction calculator will answer all your burning questions regarding how to find percent yield. Just follow the instructions below.

**Input:**

- Put the value of the actual yield
- Put the values of theoretical yield
- Press “Calculate”

**Output:**

Percentage yield calculator chemistry will give you the following results:

- Percent yield of the chemical reaction
- Step-by-step calculations

## FAQs:

### Why Is the Actual Yield Smaller Than the Theoretical Yield?

The actual yield is always smaller than the expected yield due to experimental errors and the affected factors. The factors are:

- Loss of the product
- Presence of impurities
- Some reactants escape into the air
- Some reactants don’t convert into the product
- Unwanted products are formed in a side reaction

If the actual yield equals the hypothesis yield, then the percent yield is 100%.

### Does Increasing Pressure Cause To Increase In the Yield?

Yes, increasing pressure causes the enhancement of the yield. At increasing pressure, moles of gaseous atoms decrease, equilibrium will shift in the forward direction, and the product yield will increase.

### How Do Impurities Affect the Percent Yield?

The existence of impurities decreases the actual yield. As a result, it decreases the percent yield. The purity of the reactant is the factor that affects the percentage yield. Highly pure reactants tend to increase the actual yield and the percentage yield.

### How We Increase the Percent Yield?

It is important to follow the points below to increase the percent yield of the chemical reaction.

- Use clean glass
- Evaluate the exact amount of reagents weigh
- Purify reagents and solvent
- Must use the pure reactant
- Wash flasks and syringes used to transfer the reactant

## References:

From the source Wikipedia: Annual percentage yield, Equation.

From the source Khan Academy: Limiting reactant and reaction yields, Limiting reactant and theoretical yield, Worked example, Stoichiometry.