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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