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10. The equilibrium constant Kp for the reaction (CH3),CCI (g) = (CH3),C=CH2 (g) + HCl (g) is 3.45 at 500. K. (5.00 x 10² K) Calculate the value of Kc at 500. K. For the same reaction, calculate the molar concentration of reactants and products at equilibrium if initially 1.00 mol of (CH):CCl was placed in a 5.00 L vessel.

10. The equilibrium constant Kp for the reaction (CH3),CCI (g) = (CH3),C=CH2 (g) + HCl (g) is 3.45 at 500. K. (5.00 x 10² K) Calculate the value of Kc at 500. K. For the same reaction, calculate the molar concentration of reactants and products at equilibrium if initially 1.00 mol of (CH):CCl was placed in a 5.00 L vessel.

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 56QRT
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please show the work by substituting in the quadratic equation x^2+0.0840-0.0168=0 am stuck at this thank you 

10. The equilibrium constant Kp for the reaction (CH3);CCI (g) = (CH;),C=CH2 (g) + HC1 (g) is 3.45 at 500. K. (5.00 x 10° K) Calculate the value of Kc at 500. K. For the same reaction, calculate the molar concentration of reactants and products at equilibrium if initially 1.00 mol of (CH:):CCl was placed in a 5.00 L vessel.
Transcribed Image Text:10. The equilibrium constant Kp for the reaction (CH3);CCI (g) = (CH;),C=CH2 (g) + HC1 (g) is 3.45 at 500. K. (5.00 x 10° K) Calculate the value of Kc at 500. K. For the same reaction, calculate the molar concentration of reactants and products at equilibrium if initially 1.00 mol of (CH:):CCl was placed in a 5.00 L vessel.
Expert Solution
Step 1

Given : 

Kp= 3.45 

Temperature= 500 K 

Initial moles of (CH3)3CCl = 1.00 moles 

Volume of solution = 5.0 L 

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