Volume of oxygen needed for complete combustion of 20 mL of a hydrocarbon Cx Hy will be : (a) (

step 1 volume of oxygen needed for complete combustion or 20 m of hydrocarbon CX, HY will be. So when C

Volume of oxygen needed for complete combustion of 20 mL of...

Volume of oxygen needed for complete combustion of $20 \mathrm{~mL}$ of a hydrocarbon $\mathrm{C}_{x} \mathrm{H}_{y}$ will be :
(a) $(x+y / 4) \mathrm{mL}$
$\square$ (b) $20(x+y / 4) \mathrm{mL}$
(c) $1 / 20(x+y / 4) \mathrm{mL}$
$\square$ (d) none of these

Key Concepts

Avogadro's Law

Avogadro's law states that equal volumes of gases, at the same temperature and pressure, contain an equal number of molecules. This principle allows chemists to directly relate the stoichiometric coefficients in a balanced gaseous reaction to the corresponding volumes of the gases involved, facilitating calculations in gas-phase reactions like combustion.

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction, derived from the balanced equation. It is used to determine how much of each reactant is necessary for complete reaction, such as the volume of oxygen needed to completely combust a given volume of a hydrocarbon.

Combustion Reaction

Combustion reactions involve the oxidation of a substance by oxygen, resulting in the complete conversion of the reactant to specific oxidation products. In the case of hydrocarbons, the reaction typically produces carbon dioxide and water. Understanding this reaction is essential to predict the amounts of reactants required and products formed.

Balancing Chemical Equations

Balancing chemical equations is the process of ensuring that the same number of each type of atom is present on both the reactant and product sides of the equation. This is crucial in combustion reactions to accurately relate the amounts (or volumes) of the reactants, such as the hydrocarbon and oxygen, and the resultant products.

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