Question

Suppose 5.0 g of Compound A and 5.0 g of Compound B are consumed in a reaction that produces only one product, Compound C. Calculate the theoretical yield of C. Round your answer to the nearest 0.1 g

Answer 1

To calculate the theoretical yield of compound C, determine the limiting reactant between compounds A and B by calculating the moles of each compound using their molar masses. Then, use the stoichiometric ratio between the limiting reactant and compound C to calculate the mass of compound C. Round the answer to the nearest 0.1 g.

Step-by-step explanation:

To calculate the theoretical yield of compound C, we need to determine the limiting reactant between compounds A and B. This is done by calculating the moles of each compound using their molar masses. Then, we compare the ratios of the moles to determine which reactant will be completely consumed. Once we determine the limiting reactant, we can use its ratio with compound C to calculate the theoretical yield.

Let's begin by calculating the moles of compounds A and B using their molar masses:

Moles of A = (mass of A / molar mass of A)

Moles of B = (mass of B / molar mass of B)

Next, we calculate the ratio of the moles of A to B. If the ratio is less than the stoichiometric ratio (ratio of A to B in the balanced equation), then A is the limiting reactant. Otherwise, B is the limiting reactant.

Finally, we use the stoichiometric ratio between the limiting reactant and compound C to calculate the moles and mass of compound C. To convert moles to grams, we multiply by the molar mass of compound C. The result is the theoretical yield of compound C. Round the answer to the nearest 0.1 g.