Propane (C3 H8) is a component of natural gas and is used in...

Propane $\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)$ is a component of natural gas and is used in domestic cooking and heating. (a) Balance the following equation representing the combustion of propane in air.$$\mathrm{C}_{3} \mathrm{H}_{8}+\mathrm{O}_{2} \longrightarrow \mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}$$ (b) How many grams of carbon dioxide can be produced by burning 3.65 moles of propane? Assume that oxygen is the excess reactant in this reaction.

Propane $\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)$ is a component of natural gas and is used in domestic cooking and heating.
(a) Balance the following equation representing the combustion of propane in air.$$\mathrm{C}_{3} \mathrm{H}_{8}+\mathrm{O}_{2} \longrightarrow \mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}$$
(b) How many grams of carbon dioxide can be produced by burning 3.65 moles of propane? Assume that oxygen is the excess reactant in this reaction.

Key Concepts

Stoichiometry

Stoichiometry relates the quantities of reactants and products in a chemical reaction using mole ratios derived from the balanced chemical equation. It is crucial for determining how much of each substance is consumed or produced, which is particularly useful when calculating yields or required reactant amounts in practical applications.

Molar Mass and Conversion

The concept of molar mass is used to convert between the mass of a substance and the number of moles, based on the atomic masses of the constituent elements. This conversion is key when determining the mass of products formed from a known number of moles of reactants, as it bridges the gap between the molecular scale and practical laboratory measurements.

Combustion Reactions

Combustion reactions involve a substance reacting with oxygen to produce carbon dioxide, water, and energy in the form of heat and light. These reactions are common for hydrocarbons, where the carbon and hydrogen atoms combine with oxygen during the combustion process.

Balancing Chemical Equations

Balancing chemical equations ensures that the number of atoms for each element is conserved during a reaction. This process involves adjusting coefficients so that the same types and numbers of atoms appear on both sides of the equation, which is essential for correctly representing a chemical reaction and performing subsequent calculations.

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