I don't know how to obtain theoretical yield.

To calculate the theoretical yield, you need to know the balanced chemical equation for the reaction, the stoichiometry (the ratio of reactants and products), and the amount of limiting reactant.

Here is a step-by-step process to find the theoretical yield:

1. Obtain the balanced chemical equation for the reaction. This equation indicates the reactants on the left side and the products on the right side. Make sure the equation is balanced, meaning the number of atoms of each element is the same on both sides of the equation.

2. Identify the limiting reactant. The limiting reactant is the reactant that is completely consumed in the reaction and determines the maximum amount of product that can be formed. To find the limiting reactant, compare the amounts (usually in moles) of each reactant that you have available. The reactant with the smaller amount is the limiting reactant.

3. Determine the stoichiometry of the reaction. The stoichiometry of a reaction is the balanced ratio of reactants to products. It is determined from the coefficients in the balanced chemical equation. For example, if the equation is 2A + 3B -> 4C, the stoichiometry is A:B:C = 2:3:4.

4. Calculate the moles of product that can be formed. To do this, multiply the moles of the limiting reactant by the stoichiometric ratio of the product from the balanced chemical equation. This gives you the theoretical yield of the product in moles.

5. Convert the moles of product to grams (if necessary) using the molar mass of the product. The molar mass is the mass of one mole of the substance, expressed in grams per mole. Multiply the moles of product by the molar mass to obtain the theoretical yield in grams.

It is important to note that the theoretical yield assumes perfect conditions, where there is 100% conversion of reactants to products and no side reactions or losses. In reality, actual yields may be lower due to various factors like incomplete reaction, impurities, or loss during separation processes.