Propane gas (C3 H8) reacts with oxygen to produce carbon...

Propane gas $\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)$ reacts with oxygen to produce carbon dioxide and water. $(9.2,9.3)$ $$ \mathrm{C}_{3} \mathrm{H}_{8}(g)+5 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 3 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g) $$ a. How many moles of $\mathrm{H}_{2} \mathrm{O}$ form when $5.00 \mathrm{~mol}$ of $\mathrm{C}_{3} \mathrm{H}_{8}$ completely reacts? b. How many grams of $\mathrm{CO}_{2}$ are produced from $18.5 \mathrm{~g}_{\text {of }} \mathrm{O}_{2}$ ? c. How many grams of $\mathrm{H}_{2} \mathrm{O}$ can be produced when $46.3 \mathrm{~g}$ of $\mathrm{C}_{3} \mathrm{H}_{8}$ reacts?

Propane gas $\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)$ reacts with oxygen to produce carbon dioxide and water. $(9.2,9.3)$
$$
\mathrm{C}_{3} \mathrm{H}_{8}(g)+5 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 3 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)
$$
a. How many moles of $\mathrm{H}_{2} \mathrm{O}$ form when $5.00 \mathrm{~mol}$ of $\mathrm{C}_{3} \mathrm{H}_{8}$ completely reacts?
b. How many grams of $\mathrm{CO}_{2}$ are produced from $18.5 \mathrm{~g}_{\text {of }} \mathrm{O}_{2}$ ?
c. How many grams of $\mathrm{H}_{2} \mathrm{O}$ can be produced when $46.3 \mathrm{~g}$ of $\mathrm{C}_{3} \mathrm{H}_{8}$ reacts?

Key Concepts

Limiting Reactant

The limiting reactant is the substance in a chemical reaction that is completely consumed first, limiting the amount of product that can be formed. Identifying the limiting reactant is crucial for stoichiometric calculations since it determines the maximum yield of the products.

Balanced Chemical Equations

A balanced chemical equation represents the chemical reaction with the same number of atoms for each element on both sides, ensuring the law of conservation of mass is followed. It provides the necessary stoichiometric coefficients used to relate the quantities of reactants and products in molar terms.

Mole Concept

The mole concept is a fundamental unit in chemistry that relates the mass of a substance to the number of its constituent particles. It serves as the bridge between the atomic scale and practical laboratory measurements by allowing chemists to count entities using mass.

Mole Ratios

Mole ratios are derived from the coefficients in a balanced chemical equation and are used to quantitatively relate the amounts of reactants consumed and products formed. They allow conversion between moles of one substance to moles of another in a chemical reaction.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole. It is used to convert between the mass of a substance and the number of moles, which is essential for carrying out quantitative chemical calculations.

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