Using the Theoretical Yield Calculator helps you know how much of your product to expect from a given amount of starting material. Simply enter the inputs in the input provision and tap on the calculate button to get the output in a matter of seconds with detailed work.

**Theoretical Yield Calculator: **The Theoretical Yield Calculator is a wonderful device which helps you in calculating the Theoretical yield. Also, it tells how to calculate percentage theoretical yield, as well as the theoretical yield definition and the theoretical yield formula.

You should find the theoretical yield so that you know how much of your product to expect from a given amount of starting material. The theoretical yield equation can also be used to make sure that you react with equal moles of your reactants, so no molecule is wasted.

If you ask what is Theoretical Yield? If your reaction was 100% efficient, the amount of product which will be formed would be known as Theoretical yield. It means that every molecule reacted correctly, which means no side products are formed, and at every step, no molecule was lost on the sides of the glassware. As we know that a normal reaction deals with quintillions of molecules or atoms so itâ€™s obvious that some of the molecules may get lost. So the percent yield will never be 100%.

- To calculate the theoretical yield, some important measurements are needed like the mass of the reagents, their molecular weight, and the stoichiometry of the reaction.
- Also, you need the molecular weight of the substance that you are dealing with.
- As there are many calculations, the procedure is a little bit typical. So proper attention is given to each step. A single mistake can change the whole reaction.
- By using the given formula as discussed above, calculate the value of a mole of limiting reagent. The point that should be knotted is that the unit of weight should be taken the same.

Theoretical Yield Formula

To find out the theoretical yield formula is used. To calculate such, a theoretical yield equation is brought into play. That uses a mole of the limiting reagent that takes for granted of 100% efficiency. Without wasting much time, given below is the formula for theoretical yield in a detailed form.

**Mass of product = molecular weight of the product*(moles of limiting reagent in reaction*stoichiometry of product)**

The number of products or reactants that are present in a chemical reaction is also known as stoichiometry. If no number is added in the chemical equation then the stoichiometry is one.

**Moles of limiting reagent in reaction = mass of limiting reagent / (molecular weight of limiting reagent * stoichiometry of limiting reagent)**

**Example**

**Solution:**

With the help of sodium cyanide and acetone. Here is the example of the reaction below.

Now suppose if we ignore certain solvents as given below the arrow sign. In such a case, there is no chance of limiting reagent. Also, sodium cation behaves as a spectator ion. Now, perform the reaction between 5 grams of acetone and 2 grams of cyanide. Now, what will be the theoretical yield of hydroxyacetonitrile?

- In such a case, you need to look at the limiting reagents. According to stoichiometry, one molecule of acetone reacts with one molecule of cyanide. Hence for the above equation, mass equals the product of molecular weight and number of moles.
- mass = molecular weight * moles
- On rearranging, moles= mass/ molecular weight
- Here acetone has 58 grams of weight then moles= 5/58 = 0.862 mol
- For Cyanide, molecular weight is 26 grams then mole= 2/26 = 0.0769 mol
- In the above assumption, cyanide is less in amount, and so it is a limiting reagent.
- With the help of limiting reagents, you will efficiently know the number of moles required to complete a reaction. According to the reaction, the stoichiometry of the reaction is one, and hence total moles of hydroxyacetonitrile will be 0.0769 mol.
- The equation, mass = mole * molecular weight is again in use for theoretical calculation mass.
- The molecular weight for the net hydroxyacetonitrile formed.
**Mass = 85 * 0.0769 = 6.54 grams**

Here is one basic example that we usually consider while Yield Calculations. You have to form a compound called hydroxyacetonitrile.

While experimenting, there could be 6.54 grams of hydroxyacetonitrile.

You will feel the calculators provided for various mathematical, physics, chemistry concepts extremely helpful at Chemistrycalc.Com

**1. How can you find theoretical and actual yield?**

Theoretical Yield deals with the calculation of the actual amount of product formed after limiting reagent is consumed. However, actual yield defines the actual per cent of the theoretical yield.

**2. How to get theoretical yield and percent yield?**

Theoretical yield is the numerical calculation performed to find the amount of product that can be formed. Actual yield defines the actual product formed after the reaction took place. Divide actual yield with theoretical yield and get percent yield.

**3. How to calculate yield?**

If you want to calculate the yield of the reaction, calculate its percent yield with the formula %yield = (actual yield/ theoretical yield) x 100.

**4. Can you get 100 % yield?**

It is not possible to get 100% results in yield. However, there could be many reasons. If you yield more than 100%, then that means the reaction has impurities which can cause an increase in product mass.