**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.

Chemical reaction: 2C(s) + 3H2(g) → C2H6(g) According to the question:…

Answered: Q3. Consider the reaction: 2C(s)…

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

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