A student ran the following reaction in the laboratory at 377 K:CH₂(g) + CCL (9) ⇒ 2CH₂Cl2 (9)When she introduced 0.0391 moles ofCH4 (g) and 0.0708 moles of14CCl4 (g) into a 1.00 liter container, she found the equilibrium concentration ofCCl4 (g) to be 0.0623 M.Calculate the equilibrium constant, Ko, she obtained for this reaction.Kc =

Answered: A student ran the following reaction in…

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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A student ran the following reaction in the laboratory at 377 K:
CH₂(g) + CCL (9) ⇒ 2CH₂Cl2 (9)
When she introduced 0.0391 moles of
CH4 (g) and 0.0708 moles of
14
CCl4 (g) into a 1.00 liter container, she found the equilibrium concentration of
CCl4 (g) to be 0.0623 M.
Calculate the equilibrium constant, Ko, she obtained for this reaction.
Kc =

Expert Solution

Step 1: Equilibrium constant

The equilibrium constant of any reaction is defined as the ratio of the product of concentrations of products to that of concentrations of reactants each raised to the power of their coefficient in the balanced chemical equation.

It is denoted as K_c

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