Please explain answers clearly 9. Consider the equilibrium reaction: CH₂CH2(g) + H₂O(g) = CH3CH₂OH() at 350°CA 50.0 L tank is filled with 10.0 mol of CH₂CH2(g) and 5.0 mol of H₂O(g). Once this reaction isallowed to reach equilibrium, 7.0 mol CH₂CH2(g) and 2.0 mol of H₂O(g) are present.a) How many moles of CH3CH₂OH() are present at equilibrium?Answer: 3.0 mol CH3CH₂OHb) Determine the value of the equilibrium constant?c) Another 2.5 mol of CH₂CH2(g) are added to the equilibrium mixture from part a and allowed toreach equilibrium a second time.i) Construct the full ICE chart for this reaction in terms of moles as it re-establishesequilibrium.

Answered: 9. Consider the equilibrium reaction:…

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 1ALQ: Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed...

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Please explain answers clearly

9. Consider the equilibrium reaction: CH₂CH2(g) + H₂O(g) = CH3CH₂OH() at 350°C
A 50.0 L tank is filled with 10.0 mol of CH₂CH2(g) and 5.0 mol of H₂O(g). Once this reaction is
allowed to reach equilibrium, 7.0 mol CH₂CH2(g) and 2.0 mol of H₂O(g) are present.
a) How many moles of CH3CH₂OH() are present at equilibrium?
Answer: 3.0 mol CH3CH₂OH
b) Determine the value of the equilibrium constant?
c) Another 2.5 mol of CH₂CH2(g) are added to the equilibrium mixture from part a and allowed to
reach equilibrium a second time.
i) Construct the full ICE chart for this reaction in terms of moles as it re-establishes
equilibrium.

Expert Solution

Step 1

To find the number of moles of CH3CH2OH(I) present at equilibrium, we need to use the balanced chemical equation for the reaction. The balanced equation is:

$C H_{2} C H_{2} (g) + H_{2} O (g) ⇌ C H_{3} C H_{2} O H (I)$

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