Use the following masses of reactants and products to write balanced symbol equations
46.0 g of ethanol (C2H5OH) reacts with 96.0 g of oxygen to produce 88.0 g of carbon dioxide
and 54.0 g of water.
Answers
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Chemistry: An Atoms First Approach
2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 1, Problem 34E
Textbook Problem
In a combustion reaction, 46.0 g of ethanol reacts with 96.0 g of oxygen to produce water and carbon dioxide. If 54.0 g of water is produced, what mass of carbon dioxide is produced?
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Expert Solution
Interpretation Introduction
Interpretation: The mass of the carbon dioxide produced in the given combustion reaction is to be calculated.
Concept introduction: According to the law of conservation of mass, in a chemical reaction mass of the reactants is equal to the mass of the products.
To determine: The mass of the carbon dioxide produced in the given combustion reaction.
Explanation of Solution
Given
Mass of ethnol in the reactant =46 g
Mass of oxygen in the reactant =96 g
Mass of water in the product =54 g
The law of conservation of mass states that, in a chemical reaction mass of the reactants is equal to the mass of the products.
The combustion reaction of ethanol is,
C2H5OH+3O2
→
3H2O+2CO2
Formula
The mass of reactants is calculated using the formula,
mr=mass of ethanol + mass of oxygen
Where,
mr is the mass of reactants.
Substitute the mass of ethanol and mass of oxygen in the above equation.
mr=mass of ethanol + mass of oxygen =(46+96) =142 gm (1)
The mass of products formed is calculated using the formula,