One process for the commercial production of baking soda...

One process for the commercial production of baking soda (sodium hydrogen carbonate) involves the following reaction, in which the carbon dioxide is used in its solid form ("dry ice") both to serve as a source of reactant and to cool the reaction system to a temperature low enough for the sodium hydrogen carbonate to precipitate: $$\mathrm{NaCl}(a q)+\mathrm{NH}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CO}_{2}(s) \rightarrow$$ $$\mathrm{NH}_{4} \mathrm{Cl}(a q)+\mathrm{NaHCO}_{3}(s)$$ Because they are relatively cheap, sodium chloride and water are typically present in excess. What is the expected yield of $\mathrm{NaHCO}_{3}$ when one performs such a synthesis using $10.0 \mathrm{g}$ of ammonia and $15.0 \mathrm{g}$ of dry ice, with an excess of $\mathrm{NaCl}$ and water?

One process for the commercial production of baking soda (sodium hydrogen carbonate) involves the following reaction, in which the carbon dioxide is used in its solid form ("dry ice") both to serve as a source of reactant and to cool the reaction system to a temperature low enough for the sodium hydrogen carbonate to precipitate:
$$\mathrm{NaCl}(a q)+\mathrm{NH}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CO}_{2}(s) \rightarrow$$
$$\mathrm{NH}_{4} \mathrm{Cl}(a q)+\mathrm{NaHCO}_{3}(s)$$
Because they are relatively cheap, sodium chloride and water are typically present in excess. What is the expected yield of $\mathrm{NaHCO}_{3}$ when one performs such a synthesis using $10.0 \mathrm{g}$ of ammonia and $15.0 \mathrm{g}$ of dry ice, with an excess of $\mathrm{NaCl}$ and water?

Key Concepts

Limiting Reactant

The concept of the limiting reactant is central to chemical reactions where multiple reactants are involved. It refers to the reactant that is completely consumed first, thus limiting the total amount of product that can be formed. Determining the limiting reactant involves comparing the mole ratios of the reactants as given by the balanced chemical equation to the moles available in the reaction.

Stoichiometry

Stoichiometry involves using the quantitative relationships between reactants and products in a balanced chemical equation. It allows calculation of the amount of product formed from given amounts of reactants by converting masses to moles, using the mole ratio from the balanced equation, and then converting moles back to mass if needed.

Conversion Between Mass and Moles

Converting between mass and moles is a fundamental concept in chemistry. This conversion uses the molar mass of a substance (the mass of one mole) to convert a given mass of a chemical to the corresponding number of moles, which is essential for applying stoichiometric relationships.

Theoretical Yield Calculation

The theoretical yield represents the maximum amount of product that can be formed from given reactants under ideal conditions. It is calculated by determining the moles of product formed from the limiting reactant using stoichiometry, and then converting these moles into grams using the product's molar mass.

Excess Reagents

In reactions where one or more reactants are present in quantities greater than needed (excess reagents), the product formation is limited by the amount of the limiting reactant. Recognizing excess reagents is important as they do not directly impact the theoretical yield calculation, which is wholly dependent on the limiting factor of the reaction.

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