### Combustion of Ethylene#### Reaction OverviewEthyene burns in oxygen to form carbon dioxide and water vapor:\[ \text{C}_2\text{H}_{4(g)} + 3 \text{O}_{2(g)} \rightarrow 2 \text{CO}_{2(g)} + 2 \text{H}_2\text{O}_{(g)} \]#### Problem StatementHow many liters of water can be formed if 1.25 liters of ethene are consumed in this reaction?---This chemical equation represents the combustion of ethylene (\( \text{C}_2\text{H}_4 \)) in oxygen, forming carbon dioxide (\( \text{CO}_2 \)) and water vapor (\( \text{H}_2\text{O} \)). According to the stoichiometry of the balanced equation, 1 mole of ethene reacts with 3 moles of oxygen to produce 2 moles each of carbon dioxide and water vapor. By using the ideal gas law assumptions and the stoichiometry of the reaction, you can determine the volume of water vapor produced from a given volume of ethene under the same conditions of temperature and pressure.

Answered: Image /qna-images/answer/855b995e-e1e7-4e1c-821f-bbf9be9314e0.jpg

2. Ethylene burns in oxygen to form carbon dioxide and water vapor: C2HA(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(g) How many liters of water can be formed if 1.25 liters of ethene are consumed in this reaction?

2. Ethylene burns in oxygen to form carbon dioxide and water vapor: C2HA(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(g) How many liters of water can be formed if 1.25 liters of ethene are consumed in this reaction?

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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Stoichiometry

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Question

### Combustion of Ethylene

#### Reaction Overview
Ethyene burns in oxygen to form carbon dioxide and water vapor:

\[ \text{C}_2\text{H}_{4(g)} + 3 \text{O}_{2(g)} \rightarrow 2 \text{CO}_{2(g)} + 2 \text{H}_2\text{O}_{(g)} \]

#### Problem Statement
How many liters of water can be formed if 1.25 liters of ethene are consumed in this reaction?

---

This chemical equation represents the combustion of ethylene (\( \text{C}_2\text{H}_4 \)) in oxygen, forming carbon dioxide (\( \text{CO}_2 \)) and water vapor (\( \text{H}_2\text{O} \)). According to the stoichiometry of the balanced equation, 1 mole of ethene reacts with 3 moles of oxygen to produce 2 moles each of carbon dioxide and water vapor.

By using the ideal gas law assumptions and the stoichiometry of the reaction, you can determine the volume of water vapor produced from a given volume of ethene under the same conditions of temperature and pressure.

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