Question

Magnesium sulfate reacts with barium chloride according to the following balanced equation. If 1.20g of magnesium sulfate is allowed to react with 10.0g of barium chloride in water solution, and at the end of the experiment, 1.96g of BaSO4 is obtained what is the percent yield of barium sulfate?

Answer 1

The question involves calculating the percent yield of barium sulfate in a chemical reaction. The yield is determined by comparing the actual mass of BaSO4 obtained with the theoretical mass expected from stoichiometry.

Step-by-step explanation:

The student is asking about a reaction between magnesium sulfate and barium chloride to form barium sulfate and the corresponding percent yield of barium sulfate. The percent yield can be calculated by taking the actual yield (mass of BaSO4 obtained) and dividing it by the theoretical yield (the mass of BaSO4 expected based on stoichiometry) and then multiplying by 100% to get the percentage. Here's how you calculate it:

1. Determine the number of moles of magnesium sulfate used: 1.20g divided by its molar mass (120.37 g/mol).
2. Using the stoichiometry of the reaction, determine the theoretical mass of BaSO4 that should form.
3. Then, calculate the percent yield: (1.96g obtained / theoretical yield) x 100%.

From the given data, without knowing the molar mass of barium sulfate, one cannot complete the calculation, but the student can find this information to proceed.