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C2H5OH + 302 → 2CO2 + 3H20 AH=1367KJ/mol How many grams of carbon dioxide are produced when 370. kJ of energy are used in the following reaction?

C2H5OH + 302 → 2CO2 + 3H20 AH=1367KJ/mol How many grams of carbon dioxide are produced when 370. kJ of energy are used in the following reaction?

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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**Reaction Equation:** \[ \text{C}_2\text{H}_5\text{OH} + 3\text{O}_2 \rightarrow 2\text{CO}_2 + 3\text{H}_2\text{O} \] \[ \Delta H = 1367 \text{ kJ/mol} \] **Question:** How many grams of carbon dioxide are produced when 370 kJ of energy are used in the following reaction? **Explanation:** This chemical equation represents the combustion of ethanol (\(\text{C}_2\text{H}_5\text{OH}\)) in the presence of oxygen (\(\text{O}_2\)) to produce carbon dioxide (\(\text{CO}_2\)) and water (\(\text{H}_2\text{O}\)). The enthalpy change (\(\Delta H\)) for this reaction is 1367 kJ per mole of ethanol combusted. The problem asks us to determine the mass of carbon dioxide produced when 370 kJ of energy is released by the reaction. The key steps involve using stoichiometry to relate energy changes to the amount of substance produced or consumed in the reaction.
Transcribed Image Text:**Reaction Equation:** \[ \text{C}_2\text{H}_5\text{OH} + 3\text{O}_2 \rightarrow 2\text{CO}_2 + 3\text{H}_2\text{O} \] \[ \Delta H = 1367 \text{ kJ/mol} \] **Question:** How many grams of carbon dioxide are produced when 370 kJ of energy are used in the following reaction? **Explanation:** This chemical equation represents the combustion of ethanol (\(\text{C}_2\text{H}_5\text{OH}\)) in the presence of oxygen (\(\text{O}_2\)) to produce carbon dioxide (\(\text{CO}_2\)) and water (\(\text{H}_2\text{O}\)). The enthalpy change (\(\Delta H\)) for this reaction is 1367 kJ per mole of ethanol combusted. The problem asks us to determine the mass of carbon dioxide produced when 370 kJ of energy is released by the reaction. The key steps involve using stoichiometry to relate energy changes to the amount of substance produced or consumed in the reaction.
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