Q3. Consider the reaction: 2C(s) +3H2(g) → C2H6(g) At a certain point, the H2 is being consumed a rate of -0.35moles/minute. What is the rate of C being consumed? Of ethane being produced?

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...
icon
Related questions
Question
**Question 3: Reaction Rate Analysis**

**Reaction:**  
\[ 2 \text{C}(\text{s}) + 3 \text{H}_2(\text{g}) \rightarrow \text{C}_2\text{H}_6(\text{g}) \]

At a certain point, hydrogen (\(\text{H}_2\)) is being consumed at a rate of -0.35 moles/minute. Determine the rate at which carbon (\(\text{C}\)) is being consumed and the rate at which ethane (\(\text{C}_2\text{H}_6\)) is being produced.

**Explanation:**

- The negative sign indicates consumption of \(\text{H}_2\).
- Use stoichiometry from the balanced equation:
  - For every 3 moles of \(\text{H}_2\) consumed, 2 moles of \(\text{C}\) are consumed.
  - For every 3 moles of \(\text{H}_2\) consumed, 1 mole of \(\text{C}_2\text{H}_6\) is produced. 

Calculate the rates based on these stoichiometric relationships.
Transcribed Image Text:**Question 3: Reaction Rate Analysis** **Reaction:** \[ 2 \text{C}(\text{s}) + 3 \text{H}_2(\text{g}) \rightarrow \text{C}_2\text{H}_6(\text{g}) \] At a certain point, hydrogen (\(\text{H}_2\)) is being consumed at a rate of -0.35 moles/minute. Determine the rate at which carbon (\(\text{C}\)) is being consumed and the rate at which ethane (\(\text{C}_2\text{H}_6\)) is being produced. **Explanation:** - The negative sign indicates consumption of \(\text{H}_2\). - Use stoichiometry from the balanced equation: - For every 3 moles of \(\text{H}_2\) consumed, 2 moles of \(\text{C}\) are consumed. - For every 3 moles of \(\text{H}_2\) consumed, 1 mole of \(\text{C}_2\text{H}_6\) is produced. Calculate the rates based on these stoichiometric relationships.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 4 steps

Blurred answer
Knowledge Booster
Reaction Rates
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY