In one step in the synthesis of the insecticide carbaryl...

In one step in the synthesis of the insecticide carbaryl (Sevin), naphthol reacts with phosgene as shown. $$ \mathrm{C}_{10} \mathrm{H}_{8} \mathrm{O}+\mathrm{COCl}_{2} \longrightarrow \mathrm{C}_{11} \mathrm{H}_{7} \mathrm{O}_{2} \mathrm{Cl}+\mathrm{HCl} $$ Naphthol Phosgene a. How many kilograms of $\mathrm{C}_{11} \mathrm{H}_{7} \mathrm{O}_{2} \mathrm{Cl}$ form from $2.2 \times 10^{2} \mathrm{~kg}$ of naphthol? b. If $100 . \mathrm{g}$ of naphthol and 100 . g of phosgene react, what is the theoretical yield of $\mathrm{C}_{11} \mathrm{H}_{7} \mathrm{O}_{2} \mathrm{Cl}$ ? c. If the actual yield of $\mathrm{C}_{11} \mathrm{H}_{7} \mathrm{O}_{2} \mathrm{Cl}$ in part b is $115 \mathrm{~g}$, what is the percent yield of $\mathrm{C}_{11} \mathrm{H}_{7} \mathrm{O}_{2} \mathrm{Cl}$ ?

In one step in the synthesis of the insecticide carbaryl (Sevin), naphthol reacts with phosgene as shown.
$$
\mathrm{C}_{10} \mathrm{H}_{8} \mathrm{O}+\mathrm{COCl}_{2} \longrightarrow \mathrm{C}_{11} \mathrm{H}_{7} \mathrm{O}_{2} \mathrm{Cl}+\mathrm{HCl}
$$
Naphthol Phosgene
a. How many kilograms of $\mathrm{C}_{11} \mathrm{H}_{7} \mathrm{O}_{2} \mathrm{Cl}$ form from $2.2 \times 10^{2} \mathrm{~kg}$ of naphthol?
b. If $100 . \mathrm{g}$ of naphthol and 100 . g of phosgene react, what is the theoretical yield of $\mathrm{C}_{11} \mathrm{H}_{7} \mathrm{O}_{2} \mathrm{Cl}$ ?
c. If the actual yield of $\mathrm{C}_{11} \mathrm{H}_{7} \mathrm{O}_{2} \mathrm{Cl}$ in part b is $115 \mathrm{~g}$, what is the percent yield of $\mathrm{C}_{11} \mathrm{H}_{7} \mathrm{O}_{2} \mathrm{Cl}$ ?

Key Concepts

Stoichiometry

Stoichiometry is the quantitative relationship between the reactants and products in a chemical reaction. It uses balanced chemical equations to convert between masses, moles, and numbers of molecules. In synthesis reactions and yield calculations, stoichiometry is essential for determining how much product can be formed from a given amount of reactants, using the mole ratios provided by the balanced equation.

Limiting Reagent

The limiting reagent in a chemical reaction is the reactant that is completely consumed first, thereby limiting the amount of product that can be formed. Identifying the limiting reagent requires comparing the available mole ratios of the reactants with the stoichiometric ratios from the balanced equation. It is crucial for accurate calculation of the theoretical yield, as any reactant in excess will not contribute to additional product formation once the limiting reactant is used up.

Theoretical Yield

The theoretical yield is the maximum amount of product that can be formed from the given quantities of reactants, as predicted by stoichiometry. It is calculated by determining which reactant is the limiting reagent and then using the stoichiometric ratios to convert the amount of that reagent into the amount of product. This ideal value assumes complete conversion without any losses or side reactions.

Percent Yield

Percent yield is a measure of the efficiency of a reaction, expressed as the ratio of the actual yield obtained in an experiment to the theoretical yield, multiplied by 100 percent. It accounts for the practical losses and inefficiencies often encountered in real chemical processes, indicating how close the reaction came to achieving the maximum possible product formation predicted by stoichiometry.

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