Answered: We can use Guldberg-Waage's Mass Impact…

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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We can use Guldberg-Waage's Mass Impact Act to study the following gas equilibrium: C₂H₅OH(g) ⇔ CH₃CHO(g) + H₂ (g) At temperature T = 425 °C (698 K), the equilibrium constant is estimated to be Kc = 0.0941.

a) In an experiment, a container was filled with ethanol C₂H₅OH that was evaporated to gaseous form by 425 °C until its molar concentration was 1.325 M. After some time, equilibrium had occurred after reaction equation above. What were the molar concentrations of all the gases at equilibrium?

if possible, I would like handwritten answers with calculations. Thanks :)

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b) In a company that wants to use this gas equilibrium as a source of hydrogen gas H₂, it is desired with a gas pressure of hydrogen equal to 7,850 atm. What equilibrium pressure in atm of ethanol C₂H₅OH is required to satisfy this requirement?

c) What must the initial pressure of ethanol be to meet the requirement for 7,850 atm H₂ gas at equilibrium?

Supplied: Use an S E L table to organize data and set up the expression for Kc after Guldberg-Waages mass action law for the homogeneous gas equilibrium

if possible, I would like handwritten answers with calculations. Thanks :)

At Equilibrium, molar Concentration
[H₂] = x = 0.309 M
CCHCHOI = x = 0.309 M
=
of
Concentration of gases are!
(1-325-0.309) M
1.016 M
[CH₂CH₂OH) = 1.325 -x
=

We can use Guldberg-Waage's Mass Impact Act to study the following gas equilibrium: C₂H5OH(g) →
+ H₂ (g) At temperature T = 425 °C (698 K), the equilibrium constant is estimated to be Kc =
CH3CHO(g)
0.0941.

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