The ratio of volumes of \(\mathrm{H}_{2}\) and \(\mathrm{O}_{2}\) liberated on electrolysis of water is (a) \(1: 2\) (b) \(1: 3\) (c) \(2: 1\) (d) \(3: 1\)

Understanding the concept of chemical stoichiometry is essential when exploring reactions like the electrolysis of water. Stoichiometry refers to the calculation of the quantities of reactants and products involved in a chemical reaction based on a balanced chemical equation. It's a cornerstone of chemistry because it allows chemists to predict the amounts of substances consumed and produced in a given reaction.

For instance, in the electrolysis of water, stoichiometry helps determine the molar ratio of hydrogen to oxygen gases produced. Given the balanced equation \(2 \mathrm{H_{2}O} (l) \rightarrow 2 \mathrm{H_{2}}(g) + \mathrm{O_{2}}(g)\), we interpret this as 'two moles of liquid water produces two moles of hydrogen gas and one mole of oxygen gas.' This ratio is crucial in predicting the volume and mass of gases that will be released during electrolysis.

Practical Application of Stoichiometry

Stoichiometry isn't just a theoretical concept; it has practical applications in industries like pharmaceuticals, where precise amounts of ingredients are vital. It's also useful in environmental science for tracking pollutants, and in engineering for fuel combustion processes. Getting a firm grasp of stoichiometry can help students and professionals apply these concepts in various real-world scenarios.

A balanced chemical equation is fundamental to understanding any chemical reaction, such as the electrolysis of water. It represents a reaction with the same number of atoms for each element on both sides of the equation. This is in accordance with the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction.

When we write \(2 \mathrm{H_{2}O} (l) \rightarrow 2 \mathrm{H_{2}}(g) + \mathrm{O_{2}}(g)\), this conveys that two molecules of water decompose to form two molecules of hydrogen gas and one molecule of oxygen gas. The numbers before the chemical formulas, called coefficients, are used to balance the equation, ensuring the same number of hydrogen and oxygen atoms appears on both sides.

Essence of Equation Balance

Learning to balance equations aids in developing a deeper understanding of the chemical process and the interplay of elements. It's crucial for students to recognize that every coefficient has a physical meaning, representing the relative amounts of reactants and products. Mastery of this skill is not only beneficial academically but is essential for anyone pursuing a career in the sciences or engineering.

The gas volume ratio emerges as a significant concept when examining the outcomes of gaseous reactions, like in the electrolysis of water. According to Avogadro's law, equal volumes of all gases, at the same temperature and pressure, have the same number of molecules. This principle allows us to determine the ratio of gas volumes from the balanced chemical equation.

The electrolysis reaction, \(2 \mathrm{H_{2}O} (l) \rightarrow 2 \mathrm{H_{2}}(g) + \mathrm{O_{2}}(g)\), implies that twice as much hydrogen gas (H2) is produced compared to oxygen gas (O2) under the same conditions. Therefore, the volume ratio of hydrogen to oxygen would be 2:1. This ratio is vital for applications such as fuel cell technology, where hydrogen is used as a clean fuel, and its production efficiency is key.

Understanding Gas Laws

The gas volume ratio combines the lessons of stoichiometry and gas laws. Real-world implications include calculating the required volumes for industrial chemical processes and even for students carrying out simple laboratory experiments. Grasping this concept provides a bridge between theoretical chemistry and practical experimentation.