The complete combustion of octane, C 8 H 18 , a component of gasoline, proceeds as follows: 2 C 8 H 18 (l) + 25 O 2 (g) → 16 CO 2 (g) + 18 H 2 O (g) (c) Octane has a density of 0.692 g/mL at 20 °C. How many grams of O 2 are required to burn 15.0 gal of C 8 H 18 (the capacity of an average fuel tank)?

Hello everyone. Today we have the following problem. The complete combustion of octane, a component of gasoline precedes as follows. We have problems seen that says octane has a density of 0.692 g per milliliter at 20 °C. How many grams of oxygen are required to burn 22 gallons of octane? So first, we need to calculate the mass of octane that we have. So we have the mass of octane in grams is equal to first, we have our 22 gallons and we need to multiply by the conversion factor that one gallon is equivalent to 3.7854 leaders. We then can multiply to get from liters to milliliters with the following factor conversion factor that 1 mL is equal to 10 to the negative third liters. And then lastly, we can multiply by our density which states that 1 mL is equal to 0.692 g. Our units will cancel that and we will arrive at 5 57,628 0.93 g of our octane. We then can perform a multiple ratio. So we have our 57,628 0.93 g of our octane. We first multiply by its molar mass. So we have one mole of octane is equal to eight carbons plus 18 hydrogens for 1 14.23 g. And then we multiply from moles of octane. We have one mole of octane in our chemical equation. And we see that it's like 25 miles. We have two moles, excuse me. And then we have 25 moles of our oxygen gas. One mole of our oxygen gas is equal to its smaller mass, which is 32 g of it. When we cancel out all our units and sulfur the mass of oxygen, we get 4.04 times 10 to the fifth grams. And that aligns with answer choice D and with that, we have solved the problem overall, I hope this helped. And until next time.

Ch.3 - Chemical Reactions and Reaction Stoichiometry

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Brown 14th Edition

Ch.3 - Chemical Reactions and Reaction Stoichiometry

Problem 68c

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Chapter 3, Problem 68c

The complete combustion of octane, C₈H₁₈, a component of gasoline, proceeds as follows: 2 C₈H₁₈ (l) + 25 O₂ (g) → 16 CO₂ (g) + 18 H₂O (g) (c) Octane has a density of 0.692 g/mL at 20 °C. How many grams of O₂ are required to burn 15.0 gal of C₈H₁₈ (the capacity of an average fuel tank)?

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Convert the volume of octane from gallons to milliliters using the conversion factor: 1 gallon = 3,785.41 mL.

Calculate the mass of octane using its density: mass = volume x density.

Use the balanced chemical equation to determine the molar ratio between octane (C_8H_18) and oxygen (O_2).

Calculate the moles of octane using its molar mass: moles = mass / molar mass.

Use the molar ratio to find the moles of O_2 required, then convert moles of O_2 to grams using the molar mass of O_2.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the proportions of substances involved in a reaction, which is essential for converting quantities of one substance to another. In this case, stoichiometry will help us find the amount of oxygen needed to completely combust a given volume of octane.

Density and Volume Conversion

Density is defined as mass per unit volume and is crucial for converting between the volume of a liquid and its mass. In this problem, the density of octane (0.692 g/mL) will be used to convert the volume of octane (15.0 gallons) into grams. Understanding how to convert between different units of measurement is essential for solving problems in chemistry.

Combustion Reaction

A combustion reaction is a chemical process in which a substance reacts with oxygen to produce heat and light, typically resulting in carbon dioxide and water as products. The complete combustion of octane is represented by the provided balanced equation, which indicates the specific molar ratios of octane and oxygen required. Recognizing the nature of combustion reactions is vital for understanding the energy release and reactant requirements in this scenario.

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Combustion Apparatus

Related Practice

Automotive air bags inflate when sodium azide, NaN3, rapidly decomposes to its component elements: 2 NaN31s2¡2 Na1s2 + 3 N21g2 (c) How many grams of NaN3 are required to produce 10.0 ft3 of nitrogen gas, about the size of an automotive air bag, if the gas has a density of 1.25 g/L?

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Textbook Question

The complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2 C₈H₁₈(l) + 25 O₂(g) → 16 CO₂(g) + 18 H₂O(g) (a) How many moles of O₂ are needed to burn 1.50 mol of C₈H₁₈?

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Textbook Question

The complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2 C₈H₁₈(l) + 25 O₂(g) → 16 CO₂(g) + 18 H₂O(g) (b) How many grams of O₂ are needed to burn 10.0 g of C₈H₁₈?

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Textbook Question

The complete combustion of octane, C₈H₁₈, a component of gasoline, proceeds as follows: 2 C₈H₁₈(l) + 25 O₂(g) → 16 CO₂(g) + 18 H₂O(g). (d) How many grams of CO₂ are produced when 15.0 gal of C₈H₁₈ are combusted? (d) How many grams of CO₂ are produced when 15.0 gal of C₈H₁₈are combusted?

Textbook Question

Detonation of nitroglycerin proceeds as follows: 4 C3H5N3O91l2¡ 12 CO21g2 + 6 N21g2 + O21g2 + 10 H2O1g2 (a) If a sample containing 2.00 mL of nitroglycerin 1density = 1.592 g>mL2 is detonated, how many moles of gas are produced?

The complete combustion of octane, C8H18, produces 5470 kJ of heat. Calculate how many grams of octane are required to produce 20,000 kJ of heat.

The complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2 C8H18 (l) + 25 O2 (g) → 16 CO2 (g) + 18 H2O (g) (c) Octane has a density of 0.692 g/mL at 20 °C. How many grams of O2 are required to burn 15.0 gal of C8H18 (the capacity of an average fuel tank)?

Verified Solution

Key Concepts

Stoichiometry

Density and Volume Conversion

Combustion Reaction