2. The reaction below has an equilibrium constant Kp = 2.2 x 106 at 298 K. 2COF2(g) = CO₂(g) + CF4(g) Calculate Kp for each of the following reactions and predict whether reactants or products will be favored at equilibrium. a. COF₂(g) ¹/2CO₂(g) + ¹/2CF4(9) b. 6COF₂(g) 3CO2(g) + 3CF4(g) C. 2CO2(g) + 2CF4(g) = 4COF2(g)

2. The reaction below has an equilibrium constant Kp = 2.2 x 106 at 298 K. 2COF2(g) = CO₂(g) + CF4(g) Calculate Kp for each of the following reactions and predict whether reactants or products will be favored at equilibrium. a. COF₂(g) ¹/2CO₂(g) + ¹/2CF4(9) b. 6COF₂(g) 3CO2(g) + 3CF4(g) C. 2CO2(g) + 2CF4(g) = 4COF2(g)

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.18PAE: The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures...

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