Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Suppose a 250. mL. flask is filled with 0.10 mol of Cl₂, 2.0 mol of CHCl3 and 1.0 mol of HCl. The following reaction becomes possible: Cl₂(g) + CHC1₂(g) → HCl(g) +CCl4 (g) The equilibrium constant K for this reaction is 3.83 at the temperature of the flask. Calculate the equilibrium molarity of Cl₂. Round your answer to two decimal places. M S
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Transcribed Image Text:Suppose a 250. mL. flask is filled with 0.10 mol of Cl₂, 2.0 mol of CHCl3 and 1.0 mol of HCl. The following reaction becomes possible: Cl₂(g) + CHC1₂(g) → HCl(g) +CCl4 (g) The equilibrium constant K for this reaction is 3.83 at the temperature of the flask. Calculate the equilibrium molarity of Cl₂. Round your answer to two decimal places. M S
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Step 2: Calculation of initial concentration of species.
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Step 3: Substitution of known values in equilibrium constant expression.
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Step 4: Calculation of roots of quadratic equation.
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