2. The reaction below has an equilibrium constant of Kc = 2.2 x 106 at 298 K. 2 COF2(g) → CO₂(g) + CF4(g) Calculate Kc for each of the reactions and predict whether reactants or products will be favoured at equilibrium: a. COF2(g) = 1/2 CO2(g) + ½ CF4(g) b. 2 CO₂(g) + 2 CF4(g) = 4 COF2(g) Hint: Write the corresponding Kc expression for each reaction, compare them, then calculate a numerical value of Kc.

2. The reaction below has an equilibrium constant of Kc = 2.2 x 106 at 298 K. 2 COF2(g) → CO₂(g) + CF4(g) Calculate Kc for each of the reactions and predict whether reactants or products will be favoured at equilibrium: a. COF2(g) = 1/2 CO2(g) + ½ CF4(g) b. 2 CO₂(g) + 2 CF4(g) = 4 COF2(g) Hint: Write the corresponding Kc expression for each reaction, compare them, then calculate a numerical value of Kc.

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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