Consider the reaction and its equilibrium constant.2COF2(g) CO2(g) + CFa(g)Ko = 2.20x10 (at 298 K)What is K. for this particular reaction: 2 CO2(g) + 2 CF,(g) = 4 COF (g)O Kc = 2.07x10-13%3DO K = 9.97×1012O Kc = 2.52x10-16O K. = 1.00x10 29

2COF2(g) = CO2(g) + CF4(g) K. = 2.20x106 (at 298 K) %3D What is K, for this particular reaction: 2 CO2(g) + 2 CF4(g) = 4 COF2(g) O Kc = 2.07×10-13 %3D O K = 9.97×1012 %3D O Kc = 2.52×10-16 %3D O K. = 1.00x10-29

2COF2(g) = CO2(g) + CF4(g) K. = 2.20x106 (at 298 K) %3D What is K, for this particular reaction: 2 CO2(g) + 2 CF4(g) = 4 COF2(g) O Kc = 2.07×10-13 %3D O K = 9.97×1012 %3D O Kc = 2.52×10-16 %3D O K. = 1.00x10-29

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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Question

Consider the reaction and its equilibrium constant.
2COF2(g) CO2(g) + CFa(g)
Ko = 2.20x10 (at 298 K)
What is K. for this particular reaction: 2 CO2(g) + 2 CF,(g) = 4 COF (g)
O Kc = 2.07x10-13
%3D
O K = 9.97×1012
O Kc = 2.52x10-16
O K. = 1.00x10 29

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