Equation For Combustion Of Octane | How To Balance C8H18 O2 → Co2 H2O?

Octane is a hydrocarbon and an alkane. Its chemical formula is C8H18, and its condensed structural formula is CH3(CH2)6CH3.

Let’s break down what this means. C8H18 tells us that octane has eight carbon atoms (C) and eighteen hydrogen atoms (H). The condensed structural formula, CH3(CH2)6CH3, shows the arrangement of these atoms. It tells us that there’s a chain of eight carbon atoms, with three hydrogen atoms attached to each of the first and last carbon atoms and two hydrogen atoms attached to each of the middle six carbon atoms.

Octane is a component of gasoline and is often used as a measure of a fuel’s ability to resist knocking or premature detonation. A higher octane number means the fuel is less likely to knock.

Here’s a deeper dive into octane and its formula:

Octane is a colorless liquid that’s found in crude oil. It’s a key component of gasoline, giving it the energy needed to power our vehicles.
Hydrocarbon means the molecule is made up of only hydrogen and carbon atoms.
Alkane is a specific type of hydrocarbon where all the carbon-carbon bonds are single bonds. This means each carbon atom is connected to four other atoms.
C8H18 is the molecular formula of octane. It represents the total number of each type of atom in the molecule.
CH3(CH2)6CH3 is the condensed structural formula. It shows the arrangement of the atoms in the molecule, but it doesn’t show all the individual bonds.
Octane number is a measure of a fuel’s ability to resist knocking. Higher octane numbers mean the fuel is less likely to knock. This is important because knocking can damage the engine.

You can think of octane as a simple chain of eight carbon atoms strung together. Each carbon atom in the chain has hydrogen atoms attached to it. This simple structure is what gives octane its specific properties.

The chemical equation C8H18 + O2 → CO2 + H2O represents a combustion reaction.

Combustion reactions are a type of chemical reaction that involves the rapid reaction between a substance with an oxidant, usually oxygen, to produce heat and light. In this case, C8H18 represents octane, a common component of gasoline, and O2 is oxygen from the air. The products of this reaction are carbon dioxide (CO2) and water (H2O). The heat and light released during combustion are what make flames visible and feel hot.

Octane is a hydrocarbon, meaning it is a compound composed of only hydrogen and carbon atoms. The combustion of hydrocarbons is a common process used to generate energy in many applications, such as power plants, internal combustion engines, and even campfires.

These reactions are highly exothermic, meaning they release a large amount of energy in the form of heat and light. This is why combustion reactions are used to generate power. In addition to producing heat and light, combustion reactions can also produce other products, such as carbon monoxide (CO) and nitrogen oxides (NOx), which can be harmful to the environment.

The balance of the chemical equation C8H18 + O2 → CO2 + H2O depends on the specific conditions of the reaction. However, in general, the complete combustion of octane requires a stoichiometric ratio of 25 molecules of oxygen for every 2 molecules of octane. This ratio ensures that all of the octane is completely burned and produces only carbon dioxide and water.

Combustion reactions are fascinating and important chemical reactions that are essential for many aspects of modern life. Understanding how these reactions work can help us to develop cleaner and more efficient energy technologies.

Let’s talk about the combustion reaction of iso-octane.

Iso-octane, also known as 2,2,4-trimethylpentane, is a key component of gasoline. It’s the fuel that makes our cars go! This amazing compound has a chemical formula of C8H18 and reacts with oxygen in a process called combustion. This reaction is highly exothermic, meaning it releases a lot of heat.

Here’s the balanced chemical equation for the combustion of iso-octane:

2C8H18(l) + 25O2(g) ⟶ 16CO2(g) + 18H2O(g)

Let’s break down this equation:

2C8H18(l): This represents two moles of liquid iso-octane (the “l” indicates it’s in a liquid state).
25O2(g): This represents 25 moles of gaseous oxygen (the “g” indicates it’s in a gaseous state).
16CO2(g): This represents 16 moles of gaseous carbon dioxide (the “g” indicates it’s in a gaseous state).
18H2O(g): This represents 18 moles of gaseous water (the “g” indicates it’s in a gaseous state).

This reaction is responsible for the power that drives our cars. When iso-octane burns, it combines with oxygen to produce carbon dioxide, water, and a ton of energy in the form of heat. This heat is what turns the engine’s pistons, making the wheels turn.

It’s important to note that the combustion of iso-octane can also produce some unwanted byproducts like carbon monoxide and unburned hydrocarbons. These byproducts contribute to air pollution, and that’s why we’re always working on cleaner and more efficient engines.

So, next time you fill up your car with gasoline, remember that the combustion of iso-octane is what’s making your journey possible!

Let’s talk about octane and its combustion reaction!

The complete combustion of octane, C₈H₁₈, a component of gasoline, produces carbon dioxide (CO₂) and water (H₂O) as the main products. The balanced chemical equation for this reaction is:

2 C₈H₁₈ (l) + 25 O₂ (g) → 16 CO₂ (g) + 18 H₂O (g)

This equation tells us that two molecules of octane react with 25 molecules of oxygen (O₂) to form 16 molecules of carbon dioxide and 18 molecules of water. The (l) indicates that octane is in the liquid state, while (g) indicates that oxygen, carbon dioxide, and water are in the gaseous state.

Now, let’s dive a little deeper into the fascinating world of octane and its combustion. This reaction is the foundation of how gasoline-powered engines work. When you start your car, the combustion of octane releases a significant amount of energy, which is what drives the pistons and ultimately propels your vehicle.

Here’s the breakdown of what happens:

1. Intake: Air and fuel (octane) are mixed in the engine’s cylinders.
2. Compression: The mixture is compressed, increasing its temperature and pressure.
3. Ignition: A spark plug ignites the mixture, triggering combustion.
4. Expansion: The rapid combustion creates expanding gases that drive the piston downward.
5. Exhaust: The burnt gases are expelled from the cylinder.

This cycle repeats constantly, converting the chemical energy stored in octane into mechanical energy to power the engine. And that’s how the simple reaction of octane with oxygen fuels our cars and so many other machines!

Octane has a density of 0.692 g/mL at 20 °C. This means that one milliliter of octane weighs 0.692 grams. The density of a substance is an important property that helps us understand how much mass is contained within a given volume.

Octane has the molecular formula C8H18, which means there are eight carbon and eighteen hydrogen atoms in each molecule. The empirical formula represents the simplest whole-number ratio of elements in a compound. To find the empirical formula of octane, we need to find the greatest common factor (GCD) of 8 and 18, which is 2. Dividing both subscripts in the molecular formula by 2, we get the empirical formula for octane as C4H9.

Let’s break down why this is important and how it relates to the concept of empirical formulas:

Molecular formula: This tells us the exact number of each type of atom in a molecule. For octane, C8H18, we know exactly how many carbon and hydrogen atoms make up a single octane molecule.
Empirical formula: This provides the simplest ratio of elements in a compound. While C8H18 accurately describes the composition of an octane molecule, C4H9 simplifies that ratio. This is particularly useful when you’re dealing with compounds where you don’t know the exact molecular formula, but you know the ratio of elements.

Think of it this way: You have a recipe for a cake that uses 8 cups of flour and 18 eggs. The molecular formula is like saying, “This cake needs 8 cups of flour and 18 eggs.” But the empirical formula is like saying, “This cake needs 4 cups of flour and 9 eggs for every 1 unit of cake.” The ratio is the same, but the empirical formula makes it easier to understand the basic proportions.

This concept of empirical formulas is crucial in chemistry, especially when analyzing unknown substances. You might not always know the exact molecular formula, but you can still determine the simplest ratio of elements using experimental data and ultimately figure out the compound’s identity.

You’ve probably seen (R+M)/2 on a gas pump label. This tells you the average of two important octane numbers, Research Octane Number (RON) and Motor Octane Number (MON). To get the RON, fuel is tested in an engine at idle speed with cool air and a slow engine speed.

Why two octane numbers? It’s all about understanding how gasoline behaves under different engine conditions. RON measures how well a fuel resists knocking under ideal conditions, like a smooth, easy drive. MON, on the other hand, is more demanding. It simulates high-load conditions, like accelerating uphill or towing a heavy load.

So how do these two numbers relate to the average you see on the pump? The (R+M)/2 is a simple average that gives you a good overall picture of the fuel’s knock resistance. But, remember, RON tells you about performance in ideal conditions, while MON gives you a better idea of how the fuel will handle under stress.

Think of it this way:

RON is like a calm, easygoing friend who’s always up for a relaxed hang out.
MON is like the friend who loves adrenaline and challenges, ready for anything.

By averaging these two numbers, you get a balanced picture of the fuel’s performance.

When octane burns in air, it chemically reacts with oxygen gas (O2) to produce carbon dioxide (CO2) and water (H2O). This is a combustion reaction, which is a chemical process that releases energy in the form of heat and light. The energy released by the burning of octane is what powers our cars and other engines.

The combustion of octane is a complex process that involves many steps. First, the octane molecules are broken down into smaller molecules. These smaller molecules then react with oxygen gas (O2) to produce carbon dioxide (CO2) and water (H2O). The reaction releases energy, which is what causes the flame.

The chemical equation for the combustion of octane is:

2 C8H18 + 25 O2 → 16 CO2 + 18 H2O

This equation shows that two molecules of octane react with 25 molecules of oxygen gas (O2) to produce 16 molecules of carbon dioxide (CO2) and 18 molecules of water (H2O).

The combustion of octane is an important process that provides us with energy. However, it is also a major source of pollution. The carbon dioxide (CO2) released by the combustion of octane is a greenhouse gas that contributes to climate change.

We can reduce our emissions of carbon dioxide (CO2) by using more fuel-efficient vehicles and by using alternative fuels, such as ethanol and biodiesel.

Let’s break down the mole ratio of C8H18 (octane) to CO2 (carbon dioxide).

The mole ratio of C8H18 to CO2 is 1:8. This means that for every one mole of C8H18 that reacts, eight moles of CO2 are produced.

To see this in action, imagine you have 347.2 moles of C8H18. To find out how many moles of CO2 would be produced, you would multiply the moles of C8H18 by 8. So, 347.2 moles of C8H18 would generate 2,777.6 moles of CO2.

The molar mass of CO2 is 44.01 g/mol. This means that one mole of CO2 weighs 44.01 grams. You can use this information to calculate the mass of CO2 produced in a reaction.

To help you understand this better, let’s look at the balanced chemical equation for the complete combustion of octane:

2 C8H18 + 25 O2 → 16 CO2 + 18 H2O

This equation tells us that for every two moles of C8H18 that react, sixteen moles of CO2 are produced. This confirms our mole ratio of 1:8.

Why is this mole ratio important?

Understanding the mole ratio between reactants and products in a chemical reaction is crucial for several reasons:

Predicting the amount of product formed: Knowing the mole ratio allows you to predict how much product will be formed from a given amount of reactant.
Calculating the amount of reactant needed: You can calculate how much reactant is needed to produce a desired amount of product.
Optimizing reaction conditions: Understanding mole ratios helps you optimize reaction conditions to maximize product yield and minimize waste.

In summary, the mole ratio of C8H18 to CO2 is 1:8. This ratio is fundamental in understanding the stoichiometry of the combustion reaction of octane and plays a crucial role in various chemical calculations and optimizations.

Let’s break down why the reaction of sulfur and oxygen to form sulfur dioxide (S + O2 → SO2) is indeed considered a combustion reaction.

The reaction involves sulfur (S) combining with oxygen (O2) to produce sulfur dioxide (SO2). In this process, sulfur undergoes oxidation, meaning it loses electrons and its oxidation number increases from 0 to +4. Simultaneously, oxygen undergoes reduction, gaining electrons and its oxidation number decreases from 0 to -2. This exchange of electrons makes it a redox reaction.

But what makes it a combustion reaction? Combustion reactions are characterized by:

Rapid reaction with oxygen: The reaction of sulfur and oxygen happens quickly, releasing energy in the form of heat and light.
Production of heat and light: You’ll notice a flame and heat generated when sulfur burns in air.
Formation of oxidized products: In this case, the product is sulfur dioxide (SO2), which is an oxidized form of sulfur.

So, while the reaction is definitely a redox reaction, it also meets all the criteria for a combustion reaction.

Going deeper into the combustion process:

Imagine sulfur (S) as a small, energetic molecule. It’s like a tiny ball of energy just waiting to be released. Oxygen (O2), on the other hand, is like a hungry beast ready to grab those energy balls. When sulfur and oxygen come together, they react violently. Think of it as a collision that releases a huge burst of energy—that’s the flame and heat you see.

The heat from the reaction causes more sulfur to react with oxygen, creating a chain reaction. This continues until either the sulfur or oxygen runs out. That’s why you see the flame stay lit until one of the reactants is consumed.

In essence, the combustion of sulfur is a rapid reaction between sulfur and oxygen, producing heat and light and resulting in the formation of a new compound—sulfur dioxide. It’s a fascinating example of how chemical reactions can release energy and create new substances.

Let’s dive into the fascinating world of octane combustion!

You’re likely interested in the burning reaction of octane, and that’s precisely what the chemical equation 2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O represents.

This equation, known as a balanced chemical equation, is the core of understanding how octane burns. It tells us what happens when octane (C₈H₁₈) reacts with oxygen (O₂) in the presence of a spark or flame.

Here’s the breakdown:

2C₈H₁₈ represents two molecules of octane.
25O₂ signifies twenty-five molecules of oxygen.
16CO₂ indicates sixteen molecules of carbon dioxide (CO₂) being produced.
18H₂O symbolizes eighteen molecules of water (H₂O) generated during the reaction.

Think of it this way: Octane, a component of gasoline, is like a fuel. When you ignite it, it combines with oxygen from the air, a process known as combustion. This reaction creates a burst of energy, which we observe as a flame, and releases carbon dioxide and water as byproducts.

Now, let’s delve a little deeper:

The burning reaction of octane is a complex process that involves several steps. First, the octane molecules break down into smaller fragments. Then, these fragments react with oxygen to form carbon dioxide and water. The energy released during this reaction is what drives the combustion process.

It’s important to note that this reaction produces a significant amount of heat. This heat is what powers engines in cars, allowing them to move.

Understanding the burning reaction of octane is crucial to comprehending how gasoline fuels engines and the environmental implications of its use.

Let’s talk about the burning of octane, also known as combustion. When you burn octane in the presence of plenty of oxygen, you get carbon dioxide and water. But, how much of each ingredient do you need to get a perfect burn? That’s where stoichiometry comes in.

It’s like a recipe for burning! The stoichiometric ratio between octane and oxygen is 2:25. This means for every two molecules of octane, you need 25 molecules of oxygen. Think of it like baking a cake: you need the right amount of flour, sugar, and eggs for it to turn out right.

You also have a ratio for the products – carbon dioxide and water. This ratio is 16:18. This means for every 16 molecules of carbon dioxide produced, you get 18 molecules of water.

Now, let’s get a little deeper into this.

Imagine you’re trying to burn octane, but you don’t have enough oxygen. This is called incomplete combustion. It’s like trying to bake a cake with not enough flour; you won’t get the same result. In incomplete combustion, you get less carbon dioxide and water, and you might even get some unwanted byproducts like carbon monoxide. This is why it’s important to have enough oxygen to ensure complete combustion.

Here’s a breakdown of the chemical equation for the complete combustion of octane:

2 C8H18 + 25 O2 → 16 CO2 + 18 H2O

Let’s break down this equation:

C8H18 represents octane, a hydrocarbon with 8 carbon atoms and 18 hydrogen atoms.
O2 represents oxygen, the molecule that is essential for combustion.
CO2 represents carbon dioxide, a product of complete combustion.
H2O represents water, another product of complete combustion.

The coefficients in front of each molecule represent the stoichiometric ratio:

2 molecules of octane react with 25 molecules of oxygen to produce 16 molecules of carbon dioxide and 18 molecules of water.

This equation shows that combustion is a process where octane reacts with oxygen to produce carbon dioxide and water. The stoichiometric ratio ensures that the reaction occurs in the correct proportions, leading to a complete burn and minimizing the production of harmful byproducts.

Let’s dive into the world of octane and its combustion! You’re asking about the balanced equation for the reaction of octane with oxygen. This reaction is a classic example of a combustion reaction, which is the rapid reaction between a substance with oxygen, releasing energy in the form of heat and light.

Octane, with the chemical formula C8H18, is a key component of gasoline. It’s a highly flammable alkane, which means it’s a hydrocarbon with single bonds between its carbon atoms.

The balanced chemical equation for the combustion of octane is:

2C8H18 + 25O2 → 16CO2 + 18H2O

This equation tells us that two molecules of octane react with 25 molecules of oxygen to produce 16 molecules of carbon dioxide and 18 molecules of water.

It’s crucial to balance chemical equations because they represent the law of conservation of mass. This law states that the total mass of the reactants in a chemical reaction must equal the total mass of the products.

Think of it like a recipe. You need the right amount of each ingredient (reactants) to get the desired outcome (products). In this case, the balanced equation ensures that we have the same number of carbon, hydrogen, and oxygen atoms on both sides of the equation.

Here’s how to break down the equation:

Reactants:
Octane (C8H18): This is the fuel being burned.
Oxygen (O2): This is the oxidant that supports the combustion.

Products:
Carbon Dioxide (CO2): A colorless gas produced during combustion.
Water (H2O): Another product of combustion, often seen as vapor or steam.

Now, let’s talk about why this equation is crucial for understanding how octane burns. The combustion of octane in your car’s engine provides the power to move your vehicle. The energy released from this reaction is harnessed to turn the engine’s crankshaft, which then drives the wheels.

That’s the basic idea!

Let’s talk about burning octane, a key ingredient in gasoline.

The chemical reaction that happens when octane burns completely is:

2 C 8 H 18 (l) + 25 O 2 (g) → 16 CO 2 (g) + 18 H 2 O (g)

This means that two molecules of liquid octane react with 25 molecules of oxygen gas to produce 16 molecules of carbon dioxide gas and 18 molecules of water vapor.

But how much oxygen is needed to burn a specific amount of octane, like the 15 gallons in a typical car’s fuel tank? Let’s break it down:

Octane’s density is 0.692 g/mL at 20 °C. This means that every milliliter of octane weighs 0.692 grams.

To figure out how much oxygen is needed to burn 15 gallons of octane, we need to convert gallons to milliliters:

* There are 3.785 liters in 1 gallon.
* Therefore, 15 gallons is equivalent to 15 gallons * 3.785 liters/gallon = 56.775 liters.
* There are 1000 milliliters in 1 liter, so 56.775 liters is equivalent to 56,775 milliliters.

Now that we have the volume of octane in milliliters, we can calculate its mass:

* The mass of 56,775 milliliters of octane is 56,775 mL * 0.692 g/mL = 39,312 grams.

Finally, we can use the balanced chemical equation to determine how much oxygen is needed:

* The equation tells us that 2 moles of octane react with 25 moles of oxygen.
* We need to find the molar mass of octane (C8H18) and oxygen (O2).
* The molar mass of octane is 114.23 g/mol, and the molar mass of oxygen is 32.00 g/mol.
* Using these molar masses, we can calculate the mass of oxygen needed to react with 39,312 grams of octane.

To calculate the mass of oxygen needed, we can use the following steps:

1. Convert the mass of octane to moles: 39,312 g / 114.23 g/mol = 344.3 moles of octane.
2. Use the mole ratio from the balanced chemical equation to determine the moles of oxygen needed: 344.3 moles of octane * (25 moles of oxygen / 2 moles of octane) = 4,304 moles of oxygen.
3. Convert the moles of oxygen to grams: 4,304 moles of oxygen * 32.00 g/mol = 137,728 grams of oxygen.

Therefore, you would need 137,728 grams of oxygen to completely burn 15 gallons of octane.

It’s important to understand that this calculation assumes complete combustion, which means all the octane reacts with oxygen to form carbon dioxide and water. In reality, car engines aren’t perfectly efficient, and some of the octane may not burn completely, leading to the formation of harmful byproducts like carbon monoxide.

Additionally, the combustion of octane is a complex process, involving several steps and intermediate compounds. While the balanced chemical equation gives us a simplified picture, it doesn’t capture the full complexity of what happens inside an engine cylinder. Understanding this complex process is important for engineers who design and optimize engines to improve efficiency and reduce emissions.

What Happens When Octane Combines with Oxygen?

You know how gasoline makes cars go? Well, octane is a key ingredient in gasoline! And when octane combines with oxygen, it’s a big deal. It’s called combustion, and it’s what makes your car engine roar.

Here’s the basic idea: When you burn octane, it reacts with oxygen to create carbon dioxide, water, and a whole lot of energy. That energy is what makes your car move. The chemical reaction looks like this:

2 C8H18 + 25 O2 → 16 CO2 + 18 H2O + energy

This equation means that two molecules of octane (C8H18) react with 25 molecules of oxygen (O2) to produce 16 molecules of carbon dioxide (CO2), 18 molecules of water (H2O), and a lot of energy.

This reaction is called an exothermic reaction because it releases heat. That heat is what makes the engine hot and allows the car to move. The heat also creates pressure which pushes the pistons in the engine, and that’s what makes the car go.

The combustion of octane is a pretty complex process, but the key thing to remember is that it’s a reaction between octane and oxygen that produces energy. That energy is what powers our cars, and it’s a pretty amazing thing!

Let’s dig a little deeper into why this reaction releases so much energy. The bonds between the carbon and hydrogen atoms in octane are relatively weak. When octane combines with oxygen, these bonds break, and new, stronger bonds are formed between carbon and oxygen to create carbon dioxide, and hydrogen and oxygen to create water. The difference in bond strengths releases energy, which is why the reaction is exothermic.

The amount of energy released from the combustion of octane depends on several factors, including the amount of octane and oxygen present, the temperature and pressure of the reaction, and the presence of any catalysts.

This is why it’s important to have the right mix of fuel and air in your car’s engine. Too much fuel and not enough air, and you get a smoky exhaust and poor performance. Too much air and not enough fuel, and your engine might sputter or even stall.

So, next time you’re cruising down the road, remember the amazing chemical reaction that’s powering your car! It’s all thanks to the magic of octane and oxygen!

Let’s talk about octane and how it burns! Octane, C₈H₁₈, is a component of gasoline. It’s a volatile, highly flammable alkane, meaning it’s a hydrocarbon with single bonds between the carbon atoms. When octane burns, it undergoes a combustion reaction. This means it reacts with oxygen (O₂) to produce carbon dioxide (CO₂) and water (H₂O).

Here’s the balanced chemical equation for the combustion of octane:

2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O

Let’s break down what this equation tells us:

2 C₈H₁₈: This means we need two molecules of octane for the reaction to occur.
25 O₂: We need 25 molecules of oxygen gas.
16 CO₂: The reaction produces 16 molecules of carbon dioxide.
18 H₂O: And 18 molecules of water.

This equation is balanced, which means that the same number of atoms of each element appears on both sides of the equation. This is important because it reflects the law of conservation of mass – in a chemical reaction, the total mass of the reactants must equal the total mass of the products.

Why is it important to understand the balanced chemical equation for the combustion of octane?

Understanding the products: This equation tells us that the combustion of octane produces carbon dioxide and water. Carbon dioxide is a greenhouse gas that contributes to climate change, and water vapor can also act as a greenhouse gas.
Predicting the amount of reactants and products: The balanced equation allows us to calculate the amount of reactants needed and the amount of products that will be produced in a given reaction. This is essential for chemical engineers who design and operate processes that involve combustion.
Optimizing combustion: By understanding the stoichiometry of the combustion reaction, engineers can optimize the process to maximize efficiency and minimize emissions.

Now, let’s dive into the details of balancing a chemical equation. Balancing equations isn’t just about writing down the correct formulas for reactants and products. It’s about ensuring that the same number of atoms of each element appears on both sides of the equation. This ensures that the reaction adheres to the fundamental principle of conservation of mass.

Let’s take the octane combustion equation as an example. We start with the unbalanced equation:

C₈H₁₈ + O₂ → CO₂ + H₂O

To balance this equation, we need to adjust the coefficients in front of each molecule. The coefficient represents the number of molecules of that substance involved in the reaction. We can’t change the subscripts within the formulas, as that would change the identity of the molecule.

Here’s how we balance the equation:

1. Start with carbon: There are 8 carbon atoms on the left side (in C₈H₁₈) and 1 carbon atom on the right side (in CO₂). We need to add a coefficient of 8 in front of CO₂ to balance the carbon atoms:

C₈H₁₈ + O₂ → 8 CO₂ + H₂O

2. Balance hydrogen: There are 18 hydrogen atoms on the left side (in C₈H₁₈) and 2 hydrogen atoms on the right side (in H₂O). We need to add a coefficient of 9 in front of H₂O to balance the hydrogen atoms:

C₈H₁₈ + O₂ → 8 CO₂ + 9 H₂O

3. Balance oxygen: There are 2 oxygen atoms on the left side (in O₂) and 25 oxygen atoms on the right side (16 in 8 CO₂ and 9 in 9 H₂O). We need to add a coefficient of 12.5 in front of O₂ to balance the oxygen atoms:

C₈H₁₈ + 12.5 O₂ → 8 CO₂ + 9 H₂O

However, we typically don’t use fractional coefficients in balanced chemical equations. To get whole number coefficients, we multiply the entire equation by 2:

2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O

And there you have it – the balanced chemical equation for the combustion of octane!

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