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Solved: Quantitative Information from Balanced Equations

Chemistry: A Molecular Approach | 3rd Edition | ISBN: 9780321809247 | Authors: Nivaldo J. Tro ISBN: 9780321809247 1

Solution for problem 68 Chapter 3

Chemistry: A Molecular Approach | 3rd Edition

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Chemistry: A Molecular Approach | 3rd Edition | ISBN: 9780321809247 | Authors: Nivaldo J. Tro

Chemistry: A Molecular Approach | 3rd Edition

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Problem 68

Quantitative Information from Balanced Equations (Section) The complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2 C8H18(/) + 25 O2(g)—»16 C2(g) + 18 H2O(g) (a) How many moles of O2 are needed to burn 1.50 mol of C8H18? (b) How many grams of O2 are needed to burn 10.0 g of C8H18? (c) Octane has a density of 0.692 g/ml at 20 °C. How many grams of 02 are required to burn 15.0 gal of C8H18 (the capacity of an average fuel tank)? (d) How many grams of CO2 are produced when 15.0 gal of C8H18 are combusted?

Step-by-Step Solution:
Step 1 of 3

Chapter 9 from “Introductory Chemistry” by Zumdahl and Decoste, 7 /8 editionth Pg 203. INFORMATION GIVEN BY CHEMICAL EQUATIONS *Coefficient in a balanced equation give us the relevant number of molecules Note: we need to focus on the ratio of coefficients not the specific coefficients themselves Ex: The ratio of item when making a sandwich is: 2 bread slices + 3 meat slices + 1 cheese slice...

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Chapter 3, Problem 68 is Solved
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Textbook: Chemistry: A Molecular Approach
Edition: 3
Author: Nivaldo J. Tro
ISBN: 9780321809247

The full step-by-step solution to problem: 68 from chapter: 3 was answered by , our top Chemistry solution expert on 02/22/17, 04:35PM. Since the solution to 68 from 3 chapter was answered, more than 308 students have viewed the full step-by-step answer. This full solution covers the following key subjects: burn, grams, needed, octane, gal. This expansive textbook survival guide covers 82 chapters, and 9454 solutions. The answer to “Quantitative Information from Balanced Equations (Section) The complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2 C8H18(/) + 25 O2(g)—»16 C2(g) + 18 H2O(g) (a) How many moles of O2 are needed to burn 1.50 mol of C8H18? (b) How many grams of O2 are needed to burn 10.0 g of C8H18? (c) Octane has a density of 0.692 g/ml at 20 °C. How many grams of 02 are required to burn 15.0 gal of C8H18 (the capacity of an average fuel tank)? (d) How many grams of CO2 are produced when 15.0 gal of C8H18 are combusted?” is broken down into a number of easy to follow steps, and 102 words. This textbook survival guide was created for the textbook: Chemistry: A Molecular Approach, edition: 3. Chemistry: A Molecular Approach was written by and is associated to the ISBN: 9780321809247.

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Solved: Quantitative Information from Balanced Equations

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