Answered: How many moles of CH3CH2OH(l) are…

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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Question

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(l) are present at equilibrium?

B) Determine the value of the equilibrium constant?

C) Another 2.5 mol of CH2CH2(g) is 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.
ii) Set up the equation needed to solve for x. There is no need to solve for x but use all other
known values in setting up the equation.

Expert Solution

Step 1: Given data

Given reaction:

$CH subscript 2 CH subscript 2 space plus space straight H subscript 2 straight O space rightwards arrow CH subscript 3 CH subscript 2 OH$

Initial number of moles of CH₂CH₂ = 10.0 mol

Initial number of moles of H₂O = 5.0 mol

At equilibrium,

number of moles of CH₂CH₂ = 7.0 mol

number of moles of H₂O = 2.0 mol

To calculate: number of moles of CH₃CH₂OH at equilibrium and equilibrium constant

Chemical equilibrium of a reaction is defined as the state of the reaction in which the concentration of the products and the reactants remain constant over time.

The equilibrium constant is defined as the ratio of the stoichiometric coefficient of the products to the reactants in a chemical reaction at equilibrium.

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