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Chapter 9: Problem 15

Describe the relationship between the limiting reactant and the theoretical yield.

Short Answer

Expert verified
The limiting reactant is the reactant that determines when the reaction stops as it gets used up first. The theoretical yield is the maximum output that can be theoretically produced if everything goes perfectly with no loss. The amount of product (theoretical yield) produced in a chemical reaction is directly based on the amount of the limiting reactant.

Step by step solution

01

Defining Limiting Reactant

In a chemical reaction, the limiting reactant is the substance that is entirely consumed when the reaction is complete. The limiting reactant is determined by comparing the amount of reactants used in the reaction. This reactant will limit the quantity of the product and dictate when the reaction stops as it gets used up first.
02

Defining Theoretical Yield

Theoretical yield is the quantity of a product obtained from the complete conversion of the limiting reactant in a chemical reaction. It is the maximum output that can be theoretically produced if everything goes perfectly with no loss.
03

Linking Limiting Reactant and Theoretical Yield

The relationship between the limiting reactant and theoretical yield lies in the fact that the amount of product predicted (theoretical yield) is directly based on the amount of limiting reactant. More specifically, less limiting reactant results in a lower theoretical yield, while more limiting reactant gives a higher theoretical yield, provided that there is enough of the other reactants to react completely with the limiting reactant.

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Most popular questions from this chapter

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How many grams \(\mathrm{CO}_{2}\) form from the complete combustion of \(1.00 \mathrm{L} \mathrm{C}_{8} \mathrm{H}_{18},\) density 0.700 \(\mathrm{g} / \mathrm{mL} ?\) If only \(1.90 \times 10^{3} \mathrm{g} \mathrm{CO}_{2}\) form, what is the percentage yield?

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Nitrogen monoxide, NO, reacts with oxygen to form nitrogen dioxide. Then the nitrogen dioxide reacts with oxygen to form nitrogen monoxide and ozone. Write the balanced equations. What is the theoretical yield in grams of ozone from 4.55 g of nitrogen monoxide with excess \(\mathrm{O}_{2} ?\) (Hint: First calcu- late the theoretical yield for NO \(_{2}\) , then use that value to calculate the yield for ozone.)

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