How many kilograms of CO₂ does the complete combustion of 3.8 kg of n-octane produce?

검증된 단계별 안내

Step 1: Write down the balanced chemical equation for the combustion of n-octane (C8H18). The combustion reaction of n-octane with oxygen (O2) produces carbon dioxide (CO2) and water (H2O). The balanced equation is: 2C8H18 + 25O2 -> 16CO2 + 18H2O.

Step 2: Calculate the molar mass of n-octane and CO2. The molar mass of n-octane is approximately 114.22 g/mol and the molar mass of CO2 is approximately 44.01 g/mol.

Step 3: Convert the mass of n-octane from kilograms to grams. 1 kg = 1000 g, so multiply the given mass of n-octane by 1000.

Step 4: Use the stoichiometry of the balanced chemical equation to find the moles of CO2 produced from the combustion of n-octane. From the balanced equation, we can see that 2 moles of n-octane produce 16 moles of CO2.

Step 5: Convert the moles of CO2 to mass in kilograms. First, convert the moles of CO2 to grams by multiplying by the molar mass of CO2, then convert the mass from grams to kilograms by dividing by 1000.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Combustion Reaction

A combustion reaction is a chemical process in which a substance reacts rapidly with oxygen, producing heat and light. In the case of hydrocarbons like n-octane, the products are typically carbon dioxide (CO2) and water (H2O). Understanding this reaction is essential for calculating the amount of CO2 produced from a given mass of n-octane.

Stoichiometry

Stoichiometry is the area of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. It allows us to use balanced chemical equations to determine how much of each substance is consumed or produced. In this question, stoichiometry will help convert the mass of n-octane into the mass of CO2 generated during combustion.

Molar Mass

Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol). It is crucial for converting between the mass of a substance and the number of moles, which is necessary for stoichiometric calculations. For n-octane and CO2, knowing their molar masses will enable accurate calculations of the mass of CO2 produced from the combustion of 3.8 kg of n-octane.

How many kilograms of CO2 does the complete combustion of 3.8 kg of n-octane produce?