What is how to calculate theoretical yield?

To calculate the theoretical yield of a chemical reaction, follow these steps:

Balanced Chemical Equation: Start with a properly <a href="https://www.wikiwhat.page/kavramlar/balanced%20chemical%20equation">balanced chemical equation</a>. This equation provides the stoichiometric ratios between reactants and products.
Identify the Limiting Reactant: Determine which reactant is the <a href="https://www.wikiwhat.page/kavramlar/limiting%20reactant">limiting reactant</a>. The limiting reactant is the reactant that will be completely consumed first, thus dictating the maximum amount of product that can be formed. To find it:
- Convert the mass of each reactant to moles using its molar mass (grams/mole).
- Divide the moles of each reactant by its stoichiometric coefficient from the balanced equation.
- The reactant with the smallest result is the limiting reactant.
Calculate Moles of Product: Using the stoichiometric ratio from the balanced equation, determine the number of moles of product that can be formed from the moles of the limiting reactant. For example, if the equation is A + B → C, and the limiting reactant is A, then the mole ratio (moles of C / moles of A) will tell you how many moles of C can be produced from the available moles of A.
Convert Moles of Product to Mass: Convert the moles of product to grams using the molar mass of the product (grams/mole). This calculated mass is the theoretical yield.

Formula:

Theoretical Yield (grams) = (Moles of Limiting Reactant) * (Stoichiometric Ratio of Product to Limiting Reactant) * (Molar Mass of Product)

Example:

Consider the reaction: 2H₂ + O₂ → 2H₂O

If you react 4 grams of H₂ with excess O₂, what is the theoretical yield of H₂O?

Molar mass of H₂ = 2 g/mol. Moles of H₂ = 4 g / (2 g/mol) = 2 moles.
From the balanced equation, 2 moles of H₂ produces 2 moles of H₂O. So, the stoichiometric ratio is 2/2 = 1.
Molar mass of H₂O = 18 g/mol.
Theoretical Yield of H₂O = 2 moles * 1 * 18 g/mol = 36 grams.