A gaseous hydrocarbon gives upon combustion 0.72 g of water and 3.08 g. of CO2. The empirical

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A gaseous hydrocarbon gives upon combustion 0.72 g of water...

A gaseous hydrocarbon gives upon combustion $0.72 \mathrm{~g}$ of water and $3.08 \mathrm{~g}$. of $\mathrm{CO}_{2}$. The empirical formula of the hydrocarbon is : (a) $\mathrm{C}_{2} \mathrm{H}_{4}$ (b) $\mathrm{C}_{3} \mathrm{H}_{4}$ (c) $\mathrm{C}_{6} \mathrm{H}_{5}$ (d) $\mathrm{C}_{7} \mathrm{H}_{8}$

A gaseous hydrocarbon gives upon combustion $0.72 \mathrm{~g}$ of water and $3.08 \mathrm{~g}$. of $\mathrm{CO}_{2}$. The empirical formula of the hydrocarbon is :
(a) $\mathrm{C}_{2} \mathrm{H}_{4}$
(b) $\mathrm{C}_{3} \mathrm{H}_{4}$
(c) $\mathrm{C}_{6} \mathrm{H}_{5}$
(d) $\mathrm{C}_{7} \mathrm{H}_{8}$

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Key Concepts

Mole Concept

A fundamental idea that links the mass of a substance to the number of atoms or molecules it contains. This concept is crucial in quantitative chemical analysis, enabling the conversion from measured mass units to the number of moles required for determining empirical formulas.

Combustion Analysis

A method used in chemistry to determine the composition of an unknown compound by burning it in oxygen and measuring the masses of the resulting products, typically carbon dioxide and water. This approach allows for the indirect determination of the elemental composition, especially for carbon and hydrogen in organic compounds.

Empirical Formula Determination

The process of finding the simplest whole-number ratio of atoms in a compound. In combustion analysis, the measured masses of combustion products are converted into molar amounts for carbon and hydrogen, from which the simplest atomic ratio is deduced.

Stoichiometry

A key concept that involves calculating the relationships between the quantities of reactants and products in a chemical reaction. It is integral to combustion analysis for converting masses of products into moles and maintaining balanced chemical equations.

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