Suppose of Compound and of Compound are consumed in a reaction that produces only one product, Compound . Calculate the theoretical yield of . Round your answer to the nearest . Suppose of are actually isolated at the end of the reaction. What is the percent yield of Compound

Theoretical yield  = 9.0g

Percentage yield = 67%

Note: The question is incomplete. The complete question is given below:

Suppose 2.5 g of Compound A and 6.5 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. Suppose 6.0 g of C are actually isolated at the end of the reaction What is the percent yield of Compound C? Round your answer to the nearest whole percent. x ?

Explanation:

Theoretical yield is the quantity of a product obtained from the complete conversion of the limiting reactant  into product in a chemical reaction.

The limiting reactant is a reactant that is totally consumed when a chemical reaction is completed.

From the given data, 2.5 g of Compound A and 6.5 g of Compound B are consumed in a reaction that produces only one product, Compound C. We can assume that the limiting reactant has been used in the determining the masses of A and B that would both be completely consumed to produce C.

From the law of conservation of mass, sum of the masses of reactants equals the sum of masses of products, therefore:

Theoretical yield = sum of the reacting masses

Theoretical yield  = (2.5 + 6.5) g

Theoretical yield  = 9.0g

Percentage yield = (actual yield/theoretical yield) * 100%

Percentage yield = (6.0 g / 9.0 g) * 100%

Percentage yield = 67%

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