Suppose 4.56g of CH4 and 8.67g of Cl2 were placed in a 2.00L containter at 200C where the following equilibrium is established. CH4(g)+Cl2(g)->CH3Cl(g) + HCl(g) Use thermodynamics data and other information available in the book to calculate the concentrations of all gases at equilibrium. Be sure to carry extra digits in your calculations and only round off for the final answer.
Suppose 4.56g of CH4 and 8.67g of Cl2 were placed in a 2.00L containter at 200C where the following equilibrium is established. CH4(g)+Cl2(g)->CH3Cl(g) + HCl(g) Use thermodynamics data and other information available in the book to calculate the concentrations of all gases at equilibrium. Be sure to carry extra digits in your calculations and only round off for the final answer.
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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Suppose 4.56g of CH4 and 8.67g of Cl2 were placed in a 2.00L containter at 200C where the following equilibrium is established.
CH4(g)+Cl2(g)->CH3Cl(g) + HCl(g)
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Step 1: Equilibrium constant
VIEWStep 2: Calculation for Standard Gibbs energy change for the given reaction
VIEWStep 3: Calculation for equilibrium constant
VIEWStep 4: Initial concentration of methane and chlorine gas
VIEWStep 5: ICE table for the reaction
VIEWStep 6: Value of unknown y
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