Baking soda (NaHCO 3 ) is produced on an industrial scale by...

Baking soda (NaHCO $_{3}$ ) is produced on an industrial scale by the Solvay process. A key reaction in the process is $$\mathrm{NaCl}(a q)+\mathrm{NH}_{3}(a q)+\mathrm{CO}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow$$ $$\quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \mathrm{NaHCO}_{3}(s)+\mathrm{NH}_{4} \mathrm{Cl}(a q)$$ Suppose a reaction vessel initially contains $58.5 \mathrm{kg} \mathrm{NaCl}$ $18.8 \mathrm{kg} \mathrm{NH}_{3},$ and excess $\mathrm{CO}_{2}$ and $\mathrm{H}_{2} \mathrm{O} .$ If $66 \mathrm{kg} \mathrm{NaHCO}_{3}$ is produced, what is the percent yield?

Baking soda (NaHCO $_{3}$ ) is produced on an industrial scale by the Solvay process. A key reaction in the process is
$$\mathrm{NaCl}(a q)+\mathrm{NH}_{3}(a q)+\mathrm{CO}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow$$
$$\quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \mathrm{NaHCO}_{3}(s)+\mathrm{NH}_{4} \mathrm{Cl}(a q)$$
Suppose a reaction vessel initially contains $58.5 \mathrm{kg} \mathrm{NaCl}$ $18.8 \mathrm{kg} \mathrm{NH}_{3},$ and excess $\mathrm{CO}_{2}$ and $\mathrm{H}_{2} \mathrm{O} .$ If $66 \mathrm{kg} \mathrm{NaHCO}_{3}$ is produced, what is the percent yield?

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Key Concepts

Stoichiometry

Stoichiometry involves calculating the quantitative relationships between reactants and products in a chemical reaction. It is based on the balanced chemical equation and allows chemists to predict the amounts of substances consumed and produced, making it essential for any yield calculation.

Limiting Reactant

The limiting reactant is the reactant that is completely used up first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is crucial because it dictates the theoretical yield of the reaction.

Percent Yield

Percent yield is a metric used to assess the efficiency of a chemical reaction. It is calculated by dividing the actual yield (amount of product obtained) by the theoretical yield (maximum product predicted based on stoichiometry) and multiplying by 100, thereby providing a percentage that reflects the success of the reaction.

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