**Combustion of Ethanol in Air****Ethanol (\( C_2H_6O \)) is combusted in air according to the following reaction:**\[ C_2H_6O(l) + O_2(g) \rightarrow CO_2(g) + H_2O(l) \]**Question:**How many grams of water would be produced by the complete combustion of 5.07 moles of ethanol in the presence of excess oxygen?**Explanation:**The problem involves a chemical reaction where ethanol is burned in air to produce carbon dioxide and water. This is a classic combustion reaction in chemistry. The query asks for the mass of water produced when a specific amount of ethanol is completely combusted, assuming there is more than enough oxygen available to ensure complete combustion. To solve this problem, you would need to:1. Balance the chemical equation for the reaction.2. Use stoichiometry to calculate the moles of water produced from 5.07 moles of ethanol.3. Convert moles of water to grams using the molecular weight of water.This exercise helps in understanding chemical equations, stoichiometry, and the law of conservation of mass in chemical reactions.

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Answered: w grams of water wc

Science

Chemistry

w grams of water wc

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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