Use the References t The equilibrium constant, Ke, for the following reaction is 10.5 at 350. K. 2CH2Cl2 (9) CH₁ (9) + CCL (9) Calculate the equilibrium concentrations of reactant and products when 0.245 moles of CH2Cl2 (g) are introduced into a 1.00 L vessel at 350. K. [CH₂ Cl₂]= M [CH]-[ M [CC]=[ M
Use the References t The equilibrium constant, Ke, for the following reaction is 10.5 at 350. K. 2CH2Cl2 (9) CH₁ (9) + CCL (9) Calculate the equilibrium concentrations of reactant and products when 0.245 moles of CH2Cl2 (g) are introduced into a 1.00 L vessel at 350. K. [CH₂ Cl₂]= M [CH]-[ M [CC]=[ M
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Chapter1: Chemical Foundations
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![Use the References t
The equilibrium constant, Ke, for the following reaction is 10.5 at 350. K.
2CH2Cl2 (9) CH₁ (9) + CCL (9)
Calculate the equilibrium concentrations of reactant and products when 0.245 moles of CH2Cl2 (g) are introduced into a 1.00 L vessel at 350. K.
[CH₂ Cl₂]=
M
[CH]-[
M
[CC]=[
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4ebe06b6-2dbb-4ceb-bacc-6a59bbee5e8b%2F98e77f85-e950-483f-a1d2-187f99864532%2Fhvqx3a4_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Use the References t
The equilibrium constant, Ke, for the following reaction is 10.5 at 350. K.
2CH2Cl2 (9) CH₁ (9) + CCL (9)
Calculate the equilibrium concentrations of reactant and products when 0.245 moles of CH2Cl2 (g) are introduced into a 1.00 L vessel at 350. K.
[CH₂ Cl₂]=
M
[CH]-[
M
[CC]=[
M
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