15 mL of gaseous hydrocarbon requires 45 mL of oxygen for...

15 mL of gaseous hydrocarbon requires 45 mL of oxygen for complete combustion which produces 30 mL of $\mathrm{CO}_2$ gas, measured under identical conditions. The formula of the hydrocarbon is $\mathrm{C}_x \mathrm{H}_y$. The ratio $\frac{y}{x}$ is $\qquad$

Key Concepts

Combustion Reactions

This concept involves the chemical reaction in which a fuel, often a hydrocarbon, reacts with oxygen to produce combustion products, primarily carbon dioxide and water. The understanding of combustion reactions is crucial for determining the relationships between reactants and products, especially when the chemical formula of the fuel is unknown and needs to be deduced through analysis of the reaction products.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced equation. It enables the determination of the mole ratios between substances involved, which is essential for solving problems that require finding the empirical formula of compounds, as well as for quantifying the consumption or production of chemicals during a reaction.

Avogadro's Law

Avogadro's Law states that equal volumes of gases under the same temperature and pressure contain an equal number of moles. This principle allows for the direct comparison of gas volumes as proxies for moles, which simplifies the analysis of gaseous reactions and the calculation of the chemical formula by linking measured volumes to the stoichiometric coefficients in the balanced chemical equation.

Balancing Chemical Equations

Balancing chemical equations is the process of ensuring that the number of atoms of each element is equal on both the reactant and product sides of a chemical reaction. This is critical for correctly applying stoichiometric relationships and for accurately determining the proportions of elements in compounds, which is particularly important when deducing the formula of an unknown hydrocarbon from its combustion data.

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