Chlorine dioxide, ClO2, is sometimes used as a chlorinating...

Chlorine dioxide, $\mathrm{ClO}_{2}$, is sometimes used as a chlorinating agent for water treatment. It can be prepared from the reaction below: $$\mathrm{Cl}_{2}(\mathrm{g})+4 \mathrm{NaClO}(\mathrm{aq}) \longrightarrow 4 \mathrm{NaCl}(\mathrm{aq})+2 \mathrm{ClO}_{2}(\mathrm{g})$$ In an experiment, $1.0 \mathrm{LCl}_{2}(\mathrm{g}),$ measured at $10.0^{\circ} \mathrm{C}$ and 4.66 atm, is dissolved in 0.750 L of 2.00 M $\mathrm{NaClO}(\mathrm{aq}) .$ If $25.9 \mathrm{g}$ of pure $\mathrm{ClO}_{2}$ is obtained, then what is the percent yield for this experiment?

Chlorine dioxide, $\mathrm{ClO}_{2}$, is sometimes used as a chlorinating agent for water treatment. It can be prepared from the reaction below:
$$\mathrm{Cl}_{2}(\mathrm{g})+4 \mathrm{NaClO}(\mathrm{aq}) \longrightarrow 4 \mathrm{NaCl}(\mathrm{aq})+2 \mathrm{ClO}_{2}(\mathrm{g})$$
In an experiment, $1.0 \mathrm{LCl}_{2}(\mathrm{g}),$ measured at $10.0^{\circ} \mathrm{C}$ and 4.66 atm, is dissolved in 0.750 L of 2.00 M $\mathrm{NaClO}(\mathrm{aq}) .$ If $25.9 \mathrm{g}$ of pure $\mathrm{ClO}_{2}$ is obtained, then what is the percent yield for this experiment?

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Key Concepts

Stoichiometry

Stoichiometry involves using the balanced chemical equation to relate amounts of reactants and products. It allows one to convert between moles of one substance to moles of another, using the stoichiometric coefficients given in the reaction equation, thereby connecting theoretical and experimental chemical amounts.

Limiting Reagent

The limiting reagent is the reactant that is completely consumed first in a chemical reaction, limiting the amount of product that can be formed. Identifying the limiting reagent is essential in calculating the theoretical yield, as it determines the maximum amount of product possible.

Ideal Gas Law

The ideal gas law, expressed as PV = nRT, relates the pressure, volume, temperature, and number of moles of a gas. This law is crucial for calculating the amount of a gaseous reactant or product under given conditions and integrating that information into reaction yield computations.

Percent Yield Calculation

Percent yield is a measure of the efficiency of a reaction, calculated by taking the ratio of the actual yield (the amount of product obtained experimentally) to the theoretical yield (the maximum amount predicted by stoichiometric calculations) and multiplying by 100. This concept assesses how well a reaction performed compared to its expected outcome.

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