The industrial production of hydriodic acid takes place...

The industrial production of hydriodic acid takes place bytreatment of iodine with hydrazine $\left(\mathrm{N}_{2} \mathrm{H}_{4}\right) :$ $2 \mathrm{I}_{2}+\mathrm{N}_{2} \mathrm{H}_{4} \longrightarrow 4 \mathrm{HI}+\mathrm{N}_{2}$ (a) How many grams of $\mathrm{I}_{2}$ are needed to react with 36.7 $\mathrm{g}$ of $\mathrm{N}_{2} \mathrm{H}_{4} ?$ (b) How many grams of HI are produced from the reaction of 115.7 $\mathrm{g}$ of $\mathrm{N}_{2} \mathrm{H}_{4}$ with excess iodine?

The industrial production of hydriodic acid takes place bytreatment of iodine with hydrazine
$\left(\mathrm{N}_{2} \mathrm{H}_{4}\right) :$
$2 \mathrm{I}_{2}+\mathrm{N}_{2} \mathrm{H}_{4} \longrightarrow 4 \mathrm{HI}+\mathrm{N}_{2}$
(a) How many grams of $\mathrm{I}_{2}$ are needed to react with 36.7 $\mathrm{g}$ of $\mathrm{N}_{2} \mathrm{H}_{4} ?$
(b) How many grams of HI are produced from the reaction of 115.7 $\mathrm{g}$ of $\mathrm{N}_{2} \mathrm{H}_{4}$ with excess iodine?

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Key Concepts

Limiting Reactant Concept

The limiting reactant is the substance that is entirely consumed first in a chemical reaction, thereby limiting the amount of product that can be formed. This concept is essential for accurately calculating product yields when other reactants are present in excess.

Stoichiometric Calculations

Stoichiometry involves using the mole ratios from a balanced chemical equation to determine the quantitative relationships between reactants and products. These calculations allow one to predict the amount of reactant needed to produce a desired amount of product or to calculate the yield of a product from given reactant amounts.

Molar Mass and Mole Concept

The mole concept is a central idea in chemistry that links the mass of a substance to the number of its particles. Molar mass, the mass of one mole of a substance, is used to convert between grams and moles, making it key to solving quantitative problems in chemical reactions.

Balanced Chemical Equation

A balanced chemical equation provides the relationship between reactants and products by equating the number of atoms for each element on both sides of the reaction. This balance is crucial because it establishes the mole ratios that are necessary for precise stoichiometric calculations.

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