Titanium(IV) oxide (TiO2) is a white substance produced by the action of sulfuric acid on the mi

step 1 In this problem, we want to determine our percent yield. So we have a reaction in which titanium

Titanium(IV) oxide (TiO2) is a white substance produced by...

Titanium(IV) oxide $\left(\mathrm{TiO}_{2}\right)$ is a white substance produced by the action of sulfuric acid on the mineral ilmenite $\left(\mathrm{FeTiO}_{3}\right)$ $$\mathrm{FeTiO}_{3}+\mathrm{H}_{2} \mathrm{SO}_{4} \longrightarrow\mathrm{TiO}_{2}+\mathrm{FeSO}_{4}+\mathrm{H}_{2} \mathrm{O}$$Its opaque and nontoxic properties make it suitable as a pigment in plastics and paints. In one process, $8.00 \times 10^{3} \mathrm{~kg}$ of $\mathrm{FeTiO}_{3}$ yielded $3.67 \times 10^{3} \mathrm{~kg}$ of $\mathrm{TiO}_{2} .$ What is the percent yield of the reaction?

Titanium(IV) oxide $\left(\mathrm{TiO}_{2}\right)$ is a white substance produced by the action of sulfuric acid on the mineral ilmenite $\left(\mathrm{FeTiO}_{3}\right)$
$$\mathrm{FeTiO}_{3}+\mathrm{H}_{2} \mathrm{SO}_{4} \longrightarrow\mathrm{TiO}_{2}+\mathrm{FeSO}_{4}+\mathrm{H}_{2} \mathrm{O}$$Its opaque and nontoxic properties make it suitable as a pigment in plastics and paints. In one process, $8.00 \times 10^{3} \mathrm{~kg}$ of $\mathrm{FeTiO}_{3}$ yielded $3.67 \times 10^{3} \mathrm{~kg}$ of
$\mathrm{TiO}_{2} .$ What is the percent yield of the reaction?

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Key Concepts

Mole Concept

The mole concept is a fundamental idea in chemistry that allows chemists to count entities like atoms, molecules, or formula units by linking them to measurable masses via Avogadro’s number. This concept is essential for converting masses to moles and vice versa in stoichiometric calculations.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole. It serves as a conversion factor that helps translate amounts expressed in grams to moles, enabling the accurate use of stoichiometry to calculate theoretical yields.

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction. It is defined as the ratio of the actual amount of product obtained from a reaction to the theoretical amount predicted by stoichiometric calculations, multiplied by 100. This concept is important for evaluating real-world processes where side reactions or incomplete reactions may lower the yield.

Stoichiometry

Stoichiometry involves using the balanced chemical equation to relate amounts (in moles or mass) of reactants and products. It is crucial for determining how much of a product should theoretically be produced from a given amount of reactant based solely on the reaction's coefficients.

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