In the reaction N2( g)+3 H2( g) ⇌2 NH3( g), when 100 mL of N2 has reacted, the volumes of H2 and

step 1 In this problem, 1 mole of nitrogen react with 3 moles of hydrogen to form 2 mole of ammonia. 1

In the reaction N2( g)+3 H2( g) ⇌2 NH3( g), when 100 mL of...

In the reaction $\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g})$, when 100 mL of $\mathrm{N}_2$ has reacted, the volumes of $\mathrm{H}_2$ and $\mathrm{NH}_3$ are (a) 300 mL of $\mathrm{H}_2$ and 300 mL of $\mathrm{NH}_3$ (b) 100 mL of $\mathrm{H}_2$ and 200 mL of $\mathrm{NH}_3$ (c) 300 mL of $\mathrm{H}_2$ and 200 mL of $\mathrm{NH}_3$ (d) 100 mL of $\mathrm{H}_2$ and 100 mL of $\mathrm{NH}_3$

In the reaction $\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g})$, when 100 mL of $\mathrm{N}_2$ has reacted, the volumes of $\mathrm{H}_2$ and $\mathrm{NH}_3$ are
(a) 300 mL of $\mathrm{H}_2$ and 300 mL of $\mathrm{NH}_3$
(b) 100 mL of $\mathrm{H}_2$ and 200 mL of $\mathrm{NH}_3$
(c) 300 mL of $\mathrm{H}_2$ and 200 mL of $\mathrm{NH}_3$
(d) 100 mL of $\mathrm{H}_2$ and 100 mL of $\mathrm{NH}_3$

Key Concepts

Balanced Chemical Equation

A balanced chemical equation shows the quantitative relationships between the reactants and products in a reaction. It reflects the conservation of mass by ensuring that the number of atoms of each element is equal on both the reactant and product sides, which is essential for accurately calculating how much of each substance is involved in the reaction.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on the balanced equation. It provides the quantitative relationships between substances, allowing one to determine how much of a reactant is needed or how much product will be formed from a given amount of reactant.

Mole Ratio

The mole ratio is derived from the coefficients in a balanced chemical equation and represents the proportional relationship between the moles of each reactant and product. This concept is critical in predicting the amounts of substances consumed or produced in a reaction, and it applies directly to volume, mass, and particle count calculations when conditions are consistent.

Avogadro’s Law

Avogadro’s Law states that equal volumes of all gases, at the same temperature and pressure, contain an equal number of molecules. This principle allows one to directly relate the volumes of gaseous reactants and products to their mole ratios in a chemical reaction, facilitating the use of volume measurements as proxies for moles in stoichiometric calculations.

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