Propane (C3 H8) burns in oxygen to produce carbon dioxide...

Propane $\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)$ burns in oxygen to produce carbon dioxide and water. $$ \mathrm{C}_{3} \mathrm{H}_{8}(g)+5 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 3 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g) $$ Calculate the mass of $\mathrm{CO}_{2}$ that can be produced if the reaction of $45.0 \mathrm{~g}$ of propane and sufficient oxygen has a $60.0 \%$ yield.

Propane $\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)$ burns in oxygen to produce carbon dioxide and water.
$$
\mathrm{C}_{3} \mathrm{H}_{8}(g)+5 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 3 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)
$$
Calculate the mass of $\mathrm{CO}_{2}$ that can be produced if the reaction of $45.0 \mathrm{~g}$ of propane and sufficient oxygen has a $60.0 \%$ yield.

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Key Concepts

Stoichiometry

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. It uses the mole ratios provided by a balanced chemical equation to convert between amounts (in moles) and masses, enabling the calculation of how much product is formed from a given amount of reactant.

Molar Mass

Molar mass is the mass of one mole of a substance, expressed in grams per mole. This concept is crucial for converting a substance's mass to the number of moles, a necessary step in applying stoichiometric relationships in chemical reaction calculations.

Balanced Chemical Equation

A balanced chemical equation presents the conservation of atoms in a chemical reaction by showing equal numbers of each type of atom on both the reactant and product sides. This equality allows for the use of stoichiometric coefficients to determine the mole relationships between substances.

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction, calculated as the ratio of the actual yield obtained to the theoretical yield predicted by stoichiometry, multiplied by 100. It accounts for practical losses or incomplete reactions in real-world chemical processes.

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