Iodine can be prepared by allowing an aqueous solution of...

Iodine can be prepared by allowing an aqueous solution of hydrogen iodide to react with manganese dioxide, $\mathrm{MnO}_{2}$. The reaction is $$2 \mathrm{I}^{-}(a q)+4 \mathrm{H}^{+}(a q)+\mathrm{MnO}_{2}(s) \longrightarrow \mathrm{Mn}^{2+}(a q)+2 \mathrm{H}_{2} \mathrm{O}+\mathrm{I}_{2}(s)$$ If an excess of hydrogen iodide is added to $0.200 \mathrm{~g}$ of $\mathrm{MnO}_{2}$, how many grams of iodine are obtained, assuming $100 \%$ yield?

Iodine can be prepared by allowing an aqueous solution of hydrogen iodide to react with manganese dioxide, $\mathrm{MnO}_{2}$. The reaction is
$$2 \mathrm{I}^{-}(a q)+4 \mathrm{H}^{+}(a q)+\mathrm{MnO}_{2}(s) \longrightarrow \mathrm{Mn}^{2+}(a q)+2 \mathrm{H}_{2} \mathrm{O}+\mathrm{I}_{2}(s)$$
If an excess of hydrogen iodide is added to $0.200 \mathrm{~g}$ of $\mathrm{MnO}_{2}$, how many grams of iodine are obtained, assuming $100 \%$ yield?

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Key Concepts

Balanced Chemical Equation and Stoichiometry

A balanced chemical equation provides the exact mole ratios between reactants and products, ensuring that mass and atoms are conserved during the reaction. It is the foundation for stoichiometric calculations, allowing the conversion of known quantities of one substance into expected amounts of another.

Molar Mass and Mole Conversions

Molar mass is the mass of one mole of a substance and is used to convert between mass and moles. This conversion is critical in stoichiometry, as reactions are governed by the mole relationships specified in the balanced equation.

Limiting Reagent

The limiting reagent is the reactant that is completely consumed first, thus limiting the amount of product that can be formed. Identifying the limiting reagent is essential for determining the theoretical yield in a chemical reaction.

Theoretical Yield

Theoretical yield refers to the amount of product that would be generated if the reaction proceeded perfectly, with all of the limiting reagent being converted into product. It is calculated using the mole ratios from the balanced equation and the initial amount of the limiting reagent.

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