Use average bond energies to calculate ΔH for the reaction of H2 and O2 to form water.

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
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Use average bond energies to calculate ΔH for the reaction of H2 and O2 to form water.

**Chemical Reaction: Formation of Water**

This image represents a chemical equation illustrating the formation of water from hydrogen and oxygen. The equation is balanced as follows:

\[ \text{2H}_2 + \text{O}_2 \rightarrow \text{2H}_2\text{O} \]

**Explanation:**

- **Reactants**: 
  - \( \text{2H}_2 \): Two molecules of diatomic hydrogen.
  - \( \text{O}_2 \): One molecule of diatomic oxygen.

- **Product**:
  - \( \text{2H}_2\text{O} \): Two molecules of water are produced.

**Description**:

In this chemical reaction, two molecules of hydrogen gas (\( \text{H}_2 \)) react with one molecule of oxygen gas (\( \text{O}_2 \)) to form two molecules of water (\( \text{H}_2\text{O} \)). This reaction is an example of a combustion reaction where hydrogen is burned in oxygen to produce water, releasing energy. The equation is balanced to ensure the conservation of mass, showing that the number of each type of atom is the same on both sides of the equation.
Transcribed Image Text:**Chemical Reaction: Formation of Water** This image represents a chemical equation illustrating the formation of water from hydrogen and oxygen. The equation is balanced as follows: \[ \text{2H}_2 + \text{O}_2 \rightarrow \text{2H}_2\text{O} \] **Explanation:** - **Reactants**: - \( \text{2H}_2 \): Two molecules of diatomic hydrogen. - \( \text{O}_2 \): One molecule of diatomic oxygen. - **Product**: - \( \text{2H}_2\text{O} \): Two molecules of water are produced. **Description**: In this chemical reaction, two molecules of hydrogen gas (\( \text{H}_2 \)) react with one molecule of oxygen gas (\( \text{O}_2 \)) to form two molecules of water (\( \text{H}_2\text{O} \)). This reaction is an example of a combustion reaction where hydrogen is burned in oxygen to produce water, releasing energy. The equation is balanced to ensure the conservation of mass, showing that the number of each type of atom is the same on both sides of the equation.
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