The complete combustion of octane, C8H18, 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) (a) How many moles of O 2 are needed to burn 1.50 mol of C 8 H 18 ?

Hey everyone. Our question here asked if 5.7 moles of di nitrogen Penta oxide react, how many moles of nitrogen dioxide form, Looking at our reaction, we can see that this is unbalanced. So let's go ahead and balance this out first before answering our question. So in our react inside we have two of nitrogen and five of oxygen and in our product side we have one of nitrogen And four of oxygen. Now, in order to balance this out, we're going to need to change our oxygen in our reacting side to be an even number. So we can do this by multiplying our react inside by two. Now this will change our nitrogen into four And our oxygen's into 10. Since we did this, we're going to have to balance out our product side as well. So by multiplying nitrogen dioxide by four, We end up with four of nitrogen and a total of 10 oxygen's which gives us our balanced chemical equation. Now we can go ahead and move on with our question. Starting off with 5.7 mol of di nitrogen Penta oxide, we can see that in our balance chemical reaction We have two moles of di nitrogen Penta oxide and this is equivalent to formals of nitrogen dioxide. Now, when we calculate this out, We end up with a total of 22.8 mole of nitrogen dioxide, Which we can round up to 23 and this is going to be our final answer. So I hope this made sense and let us know if you have any questions

Ch.3 - Chemical Reactions and Reaction Stoichiometry

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Brown 14th Edition

Ch.3 - Chemical Reactions and Reaction Stoichiometry

Problem 68a

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Chapter 3, Problem 68a

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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Identify the balanced chemical equation for the combustion of octane: \(2 \text{C}_8\text{H}_{18} + 25 \text{O}_2 \rightarrow 16 \text{CO}_2 + 18 \text{H}_2\text{O}\).

Determine the mole ratio between \(\text{C}_8\text{H}_{18}\) and \(\text{O}_2\) from the balanced equation. The ratio is 2 moles of \(\text{C}_8\text{H}_{18}\) to 25 moles of \(\text{O}_2\).

Set up a proportion to find the moles of \(\text{O}_2\) needed for 1.50 moles of \(\text{C}_8\text{H}_{18}\): \(\frac{2 \text{ moles C}_8\text{H}_{18}}{25 \text{ moles O}_2} = \frac{1.50 \text{ moles C}_8\text{H}_{18}}{x \text{ moles O}_2}\).

Solve the proportion for \(x\) to find the moles of \(\text{O}_2\) required.

Verify the calculation by checking the units and ensuring the mole ratio is correctly applied.

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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 branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows chemists to calculate how much of each substance is needed or produced in a reaction based on balanced chemical equations. Understanding stoichiometry is essential for solving problems involving the amounts of reactants and products.

Balanced Chemical Equation

A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. In the combustion of octane, the equation shows the ratio of octane to oxygen and the products formed. This balance is crucial for determining the exact amounts of reactants needed for a complete reaction.

Mole Concept

The mole concept is a fundamental principle in chemistry that defines a mole as 6.022 x 10^23 particles (atoms, molecules, etc.). It provides a bridge between the atomic scale and macroscopic quantities, allowing chemists to count particles by weighing them. In this question, the mole concept is used to relate the amount of octane to the required amount of oxygen for combustion.

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Mole Concept

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Calcium hydride reacts with water to form calcium hydroxide and hydrogen gas. (b) How many grams of calcium hydride are needed to form 4.500 g of hydrogen?

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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) (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) (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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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?

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?

Verified Solution

Key Concepts

Stoichiometry

Balanced Chemical Equation

Mole Concept

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?