How many grams of NH3 form when 24.8 L of H2( g) (measured...

How many grams of $\mathrm{NH}_{3}$ form when $24.8 \mathrm{~L}$ of $\mathrm{H}_{2}(\mathrm{~g})$ (measured at STP) reacts with $\mathrm{N}_{2}$ to form $\mathrm{NH}_{3}$ according to this reaction?
$$
\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)
$$

Key Concepts

Balanced Chemical Equation

A balanced chemical equation represents the reaction with equal numbers of each type of atom on both sides, ensuring the law of conservation of mass is maintained. It shows the stoichiometric relationships between reactants and products, which is essential for calculating how much product will form based on a given amount of reactant.

Mole Concept

The mole is a fundamental unit in chemistry used to quantify the amount of a substance. It provides a bridge between the microscopic world of atoms and molecules and the macroscopic world, allowing chemists to count particles by weighing them.

Stoichiometry

Stoichiometry involves the calculation of the quantitative relationships between reactants and products in a chemical reaction. It relies on the mole ratios derived from the balanced chemical equation to determine the amounts of substances consumed and produced.

Molar Volume at STP

At Standard Temperature and Pressure (STP), one mole of an ideal gas occupies 22.4 liters. This relationship allows for the conversion between the volume of a gas and the number of moles, which is crucial when dealing with gas calculations in chemical reactions.

Molar Mass

Molar mass, expressed in grams per mole (g/mol), is the mass of one mole of a substance. It is used to convert between the amount in moles and the mass in grams, facilitating the calculation of how much of a substance is present or required in a reaction.

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