Sodium and nitrogen combine to form sodium nitride....

Sodium and nitrogen combine to form sodium nitride. $(9.2,9.3$, $9.4,9.5)$ $$ 6 \mathrm{Na}(s)+\mathrm{N}_{2}(g) \longrightarrow 2 \mathrm{Na}_{3} \mathrm{~N}(s) $$ a. If $80.0 \mathrm{~g}$ of $\mathrm{Na}$ is mixed with $20.0 \mathrm{~g}$ of nitrogen gas, what is the theoretical yield, in grams, of $\mathrm{Na}_{3} \mathrm{~N}$ ? b. If the reaction in part a has a percent yield of $75.0 \%$, what is the actual yield, in grams, of $\mathrm{Na}_{3} \mathrm{~N}$ ?

Sodium and nitrogen combine to form sodium nitride. $(9.2,9.3$, $9.4,9.5)$
$$
6 \mathrm{Na}(s)+\mathrm{N}_{2}(g) \longrightarrow 2 \mathrm{Na}_{3} \mathrm{~N}(s)
$$
a. If $80.0 \mathrm{~g}$ of $\mathrm{Na}$ is mixed with $20.0 \mathrm{~g}$ of nitrogen gas, what is the theoretical yield, in grams, of $\mathrm{Na}_{3} \mathrm{~N}$ ?
b. If the reaction in part a has a percent yield of $75.0 \%$, what is the actual yield, in grams, of $\mathrm{Na}_{3} \mathrm{~N}$ ?

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Key Concepts

Percent Yield

Percent yield is the ratio of the actual yield (the quantity of product actually obtained) to the theoretical yield, multiplied by 100. It provides a measure of reaction efficiency, accounting for practical factors such as side reactions, incomplete reactions, and losses during product recovery.

Theoretical Yield

The theoretical yield is the maximum amount of product that can be produced from a given set of reactants, assuming complete conversion based on stoichiometric ratios from the balanced equation. It represents an ideal scenario where reactions proceed with 100% efficiency without any losses.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus limiting the amount of product that can be formed. Identifying the limiting reactant is crucial for accurately calculating the theoretical yield, as it dictates the maximum quantity of product achievable under given conditions.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions using the mole concept and balanced chemical equations. It allows the determination of how much of each substance is needed or produced, serving as a fundamental tool in predicting reaction yields and guiding laboratory procedures.

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