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Consider the following balanced equation for the combustion of butane, a fuel often used in lighters. 2 C4H10 (9) + 13 O2 (g) → 8 CO2 (g) + 10 H2O (g) Complete the following table, showing the appropriate masses of reactants and products. If the mass of a reactant is provided, fill in the mass of other reactants required to completely react with the given mass, as well as the mass of each product formed. If the mass of a product is provided, fill in the required masses of each reactant to make that amount of product, as well as the mass of the other product that is formed. Mass C4H10 Mass O2 Mass CO2 Mass H2O 1.11 g 5.72 g 18.12 g 9.64 g 192 mg 168 mg

Consider the following balanced equation for the combustion of butane, a fuel often used in lighters. 2 C4H10 (9) + 13 O2 (g) → 8 CO2 (g) + 10 H2O (g) Complete the following table, showing the appropriate masses of reactants and products. If the mass of a reactant is provided, fill in the mass of other reactants required to completely react with the given mass, as well as the mass of each product formed. If the mass of a product is provided, fill in the required masses of each reactant to make that amount of product, as well as the mass of the other product that is formed. Mass C4H10 Mass O2 Mass CO2 Mass H2O 1.11 g 5.72 g 18.12 g 9.64 g 192 mg 168 mg

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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VExercise 8.40: Problems - Mass-to-Mass Conversions Consider the following balanced equation for the combustion of butane, a fuel often used in lighters. 2 C4H10 (9) + 13 02 (g) →8 CO2 (g) + 10 H2O (g) Complete the following table, showing the appropriate masses of reactants and products. If the mass of a reactant is provided, fill in the mass of other reactants required to completely react with the given mass, as well as the mass of each product formed. If the mass of a product is provided, fill in the required masses of each reactant to make that amount of product, as well as the mass of the other product that is formed. Mass C4H10 Mass O2 Mass CO2 Mass H20 1.11 g 5.72 g 18.12 g 9.64 g 192 mg 168 mg
Transcribed Image Text:VExercise 8.40: Problems - Mass-to-Mass Conversions Consider the following balanced equation for the combustion of butane, a fuel often used in lighters. 2 C4H10 (9) + 13 02 (g) →8 CO2 (g) + 10 H2O (g) Complete the following table, showing the appropriate masses of reactants and products. If the mass of a reactant is provided, fill in the mass of other reactants required to completely react with the given mass, as well as the mass of each product formed. If the mass of a product is provided, fill in the required masses of each reactant to make that amount of product, as well as the mass of the other product that is formed. Mass C4H10 Mass O2 Mass CO2 Mass H20 1.11 g 5.72 g 18.12 g 9.64 g 192 mg 168 mg
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