Without doing detailed calculations, explain which of these...

Without doing detailed calculations, explain which of these compounds produces the greatest mass of $\mathrm{H}_{2} \mathrm{O}$ when $1.00 \mathrm{g}$ of the compound is burned in an excess of oxygen: $\mathrm{CH}_{4}, \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}, \mathrm{C}_{10} \mathrm{H}_{8}, \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}$.

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Key Concepts

Molar Mass

Molar mass is a measure of the mass of one mole of a substance. When comparing different compounds with the same mass (e.g., 1.00 g), compounds with smaller molar masses yield more moles, which in turn can produce a greater amount of product if the mole ratio to the product is favorable.

Mole Ratio

The mole ratio, derived from the coefficients in the balanced chemical equation, tells us the proportional relationship between the reactants and the products. This concept is key for determining how many moles of water are produced per mole of the burning compound.

Stoichiometry

Stoichiometry involves the quantitative relationships in chemical reactions between reactants and products. It allows one to determine how many moles of products are formed from a given number of moles of a reactant, based on the balanced chemical equation.

Combustion Reactions

Combustion reactions are specific chemical reactions where a substance, typically containing carbon and hydrogen, reacts with oxygen to produce combustion products such as water and carbon dioxide. Understanding the balanced equation for combustion is essential to determine the ratio in which products are formed.

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