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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 :)

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 :)

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter12: Gaseous Chemical Equilibrium
Section: Chapter Questions
Problem 13QAP: Consider the following reaction at 250C: A(s)+2B(g)C(s)+2D(g) (a) Write an equilibrium constant...
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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 =
Transcribed Image Text: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.
Transcribed Image Text: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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