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Chapter 9: Problem 43

What is the theoretical yield for a reaction, and how does this quantity depend on the limiting reactant?

Short Answer

Expert verified
The theoretical yield for a reaction is the maximum amount of product that can be produced based on the stoichiometry of the balanced chemical equation. It depends on the limiting reactant, which is the reactant that is consumed first and thus determines the maximum amount of product that can be formed. In the example provided, the limiting reactant is B, and the theoretical yield for product C is 10 moles.

Step by step solution

01

Identify the limiting reactant

First, we need to determine the limiting reactant by comparing the amount of each reactant to the stoichiometry given in the balanced chemical equation. In this case, for every 1 mole of A, we need 2 moles of B. Divide the number of moles of each reactant by their respective stoichiometric coefficients: \(A: \frac{16}{1} = 16\) \(B: \frac{20}{2} = 10\) The smaller number indicates the limiting reactant, which in this case is B.
02

Calculate the theoretical yield

Now that we have determined the limiting reactant, we can calculate the theoretical yield of product C based on the stoichiometry of the balanced chemical equation. From the balanced equation, we know that 1 mole of A reacts with 2 moles of B to form 1 mole of C. Since B is the limiting reactant, we can use the moles of B to determine the maximum moles of C that can be produced. Use the coefficients from the balanced equation to convert moles of B to moles of C: \(moles \ of \ C = (\frac{1 \ mol \ of \ C}{2 \ mol \ of \ B}) \times moles \ of \ B\) Plug in the number of moles we had at the beginning (20 moles of B): \(moles \ of \ C = (\frac{1}{2}) \times 20\) Calculate the moles of C: \(moles \ of \ C = 10\) So, the theoretical yield for product C in this reaction is 10 moles. This quantity depends on the limiting reactant, which in this case is B.

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Most popular questions from this chapter

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