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.
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.
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text: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:
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