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Ch.3 - Chemical Reactions and Reaction Stoichiometry
Chapter 3, Problem 68a

The complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2 C8H181l2 + 25 O21g2¡16 CO21g2 + 18 H2O1g2 (a) How many moles of O2 are needed to burn 1.50 mol of C8H18?

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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.
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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.
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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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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 C8H181l2 + 25 O21g2¡16 CO21g2 + 18 H2O1g2 (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

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?

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