CH4(g) + CCI4(g) 2CH2C12(g) When she introduced 4.30x10-2 moles of CH4(g) and 7.96x10-2 moles of CCI4(g) into a 1.00 liter container, she found the equilibrium concentration of CH2CI2(g) to be 2.04×10-2 M. Calculate the equilibrium constant, Ke, she obtained for this reaction.
CH4(g) + CCI4(g) 2CH2C12(g) When she introduced 4.30x10-2 moles of CH4(g) and 7.96x10-2 moles of CCI4(g) into a 1.00 liter container, she found the equilibrium concentration of CH2CI2(g) to be 2.04×10-2 M. Calculate the equilibrium constant, Ke, she obtained for this reaction.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section15.4: Using Equilibrium Constants In Calculations
Problem 15.5CYU: The decomposition of PCl5(g) to form PCl3(g) and Cl2(g) has Kc = 33.3 at a high temperature. If the...
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Question
![A student ran the following reaction in the laboratory at 389 K:
CH4(9) + CCI4(g)
?
2CH2CI2(9)
When she introduced 4.30x10-2 moles of CH4(g) and 7.96x10-2 moles of CCI4(g) into a 1.00 liter container, she found the equilibrium concentration of
CH2CI2(g) to be 2.04x10-2 M.
Calculate the equilibrium constant, Kc, she obtained for this reaction.
Kc
%D](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F491c171b-5062-4366-aa21-6fc1a28840ea%2Fac795eac-55c3-45ed-83f0-c7a7ddc2338f%2Fdwcwxt_processed.png&w=3840&q=75)
Transcribed Image Text:A student ran the following reaction in the laboratory at 389 K:
CH4(9) + CCI4(g)
?
2CH2CI2(9)
When she introduced 4.30x10-2 moles of CH4(g) and 7.96x10-2 moles of CCI4(g) into a 1.00 liter container, she found the equilibrium concentration of
CH2CI2(g) to be 2.04x10-2 M.
Calculate the equilibrium constant, Kc, she obtained for this reaction.
Kc
%D
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