Final answer:
The Correct option is 3). To find how many grams of bromine are required to produce 4.08 grams of bromine monochloride with an 82.9% yield, calculate the theoretical yield and use stoichiometry based on the balanced reaction equation.
Step-by-step explanation:
The student's question asks how many grams of bromine would be required to produce 4.08 grams of bromine monochloride (BrCl), given that the percent yield is 82.9%. To answer this, you would first calculate the theoretical yield, which represents 100% yield. Since the actual yield is 4.08 grams and the percent yield is 82.9%, the theoretical yield can be calculated as:
Theoretical Yield = Actual Yield / Percent Yield × 100%
= 4.08 g / 0.829
= 4.92 grams
This is the amount of bromine monochloride that should have been produced if the reaction had gone to completion. To find out how many grams of bromine are needed, you would use the stoichiometry of the balanced chemical equation for the reaction. Assuming that the reaction is Br2 + Cl2 → 2BrCl, it can be understood that one mole of bromine reacts to form two moles of bromine monochloride. Thus, the molar mass of bromine (Br2) allows you to determine the number of grams of bromine that correspond to the theoretical yield of bromine monochloride.