### Methane and Water Reaction to Form Carbon Monoxide and HydrogenWhen methane (CH₄) and water (H₂O) react, they form carbon monoxide (CO) and hydrogen (H₂) according to the following equation:\[ \text{CH}_4(g) + \text{H}_2\text{O}(g) \rightarrow \text{CO}(g) + 3\text{H}_2(g) \]Imagine 159. mmol of CH₄ and 159. mmol of H₂O are added to an empty flask, and then answer the following questions:---This reaction is a classic example of a steam reforming process, which is frequently used in industrial applications to produce hydrogen gas. It's valuable to depict the stoichiometry here, showing the direct mole-to-mole relationship between reactants and products for educational clarity. By understanding this, students can better grasp the conservation of mass and the concept of limiting reactants. **Chemical Reaction Equilibrium Quiz**This section contains multiple-choice questions regarding the rates of forward and reverse reactions observed in a closed system before and after CH4 and H2O have been added, as well as at equilibrium. Finally, the questions assess the amount of CH4 present in the flask at equilibrium.**Questions:**1. **What is the rate of the forward reaction before any CH4 or H2O has been added to the flask?** - O Zero. - O Greater than zero, but less than the rate of the reverse reaction. - O Greater than zero, and equal to the rate of the reverse reaction. - O Greater than zero, and greater than the rate of the reverse reaction.2. **What is the rate of the forward reaction just after the CH4 and H2O have been added to the flask?** - O Zero. - O Greater than zero, but less than the rate of the reverse reaction. - O Greater than zero, and equal to the rate of the reverse reaction. - O Greater than zero, and greater than the rate of the reverse reaction.3. **What is the rate of the forward reaction at equilibrium?** - O Zero. - O Greater than zero, but less than the rate of the reverse reaction. - O Greater than zero, and equal to the rate of the reverse reaction. - O Greater than zero, and greater than the rate of the reverse reaction.4. **How much CH4 is in the flask at equilibrium?** - O None. - O Some, but less than 159. mmol. - O 159. mmol. - O More than 159. mmol.**Explanation of Diagram:**No diagrams or graphs are present in the image provided. The content is exclusively textual in nature, focusing on multiple-choice questions related to reaction rates in a chemical equilibrium context.

Here we have to determine the rate of forward and backward reaction at different times like before…

What is the rate of the forward reaction before any CH4 or H₂O has been added to the flask? What is the rate of the forward reaction just after the CH4 and H₂O has been added to the flask? What is the rate of the forward reaction at equilibrium? How much CH4 is in the flask at equilibrium? Zero. Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. Zero. Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. Zero. Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. None. Some, but less than 159. mmol. 159. mmol.. More than 159. mmol.

What is the rate of the forward reaction before any CH4 or H₂O has been added to the flask? What is the rate of the forward reaction just after the CH4 and H₂O has been added to the flask? What is the rate of the forward reaction at equilibrium? How much CH4 is in the flask at equilibrium? Zero. Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. Zero. Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. Zero. Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. None. Some, but less than 159. mmol. 159. mmol.. More than 159. mmol.

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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### Methane and Water Reaction to Form Carbon Monoxide and Hydrogen

When methane (CH₄) and water (H₂O) react, they form carbon monoxide (CO) and hydrogen (H₂) according to the following equation:

\[ \text{CH}_4(g) + \text{H}_2\text{O}(g) \rightarrow \text{CO}(g) + 3\text{H}_2(g) \]

Imagine 159. mmol of CH₄ and 159. mmol of H₂O are added to an empty flask, and then answer the following questions:

---

This reaction is a classic example of a steam reforming process, which is frequently used in industrial applications to produce hydrogen gas. It's valuable to depict the stoichiometry here, showing the direct mole-to-mole relationship between reactants and products for educational clarity. By understanding this, students can better grasp the conservation of mass and the concept of limiting reactants.

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Step 1: Equilibrium reaction

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Step 5: Concentration of methane.

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