Final answer:
The theoretical yield is calculated using stoichiometry from a balanced chemical equation. Without the chemical formulas of the reactants, we cannot calculate a numerical value for the theoretical yield of Compound C. The process involves converting mass to moles, determining the limiting reactant, and calculating the product's mass from the balanced equation.
Step-by-step explanation:
To calculate the theoretical yield of a compound in a chemical reaction, we use stoichiometry based on the balanced chemical equation of the reaction. Given the mass of reactants, we find the molar mass of each, convert the masses to moles, and use the mole ratio to determine the limiting reactant. The limiting reactant is the one that will run out first, dictating the maximum amount of product that can be formed. This maximum amount is the theoretical yield of the reaction.
With 9.5 g of Compound A and 3.0 g of Compound B reacting to produce Compound C in a 1:1 molar ratio (as inferred from the question), to find the theoretical yield, we need the chemical formulae of the reactants or the product. Since this information is not provided in the question, we cannot calculate an exact value for the theoretical yield of Compound C. However, we can describe the process as follows:
- Determine the molar mass of Compounds A and B from their chemical formulas.
- Convert the given masses of the reactants to moles by dividing by their respective molar masses.
- Determine the limiting reactant by comparing the mole ratios of the reactants to those in the balanced equation.
- Calculate the moles of Compound C produced using the mole ratio from the balanced equation.
- Find the mass of Compound C by multiplying the moles of Compound C by its molar mass.
The actual yield is the amount of product actually obtained from a reaction. The percent yield is a measure of the efficiency of the reaction, calculated by dividing the actual yield by the theoretical yield and multiplying by 100%. Factors such as side reactions, incomplete reactions, and difficulties in product recovery can affect the actual yield and thus, the percent yield.
In the absence of exact chemical equations and formulae for the compounds in the question, we cannot provide a numerical answer for the theoretical yield of Compound C. Nonetheless, the outlined process applies when all necessary chemical information is available.