Question #19479
6. Consider the following reactions:
NO2(g) ↔ NO(g) + O(g) Kc = 4.7 x 10-42
NO(g) + O3(g) ↔ NO2(g) + O2(g) Kc = 5.3 x 10-33
Based on this information, calculate Kc for the reaction: O2(g) + O(g) ↔ O3(g)
NO2(g) ↔ NO(g) + O(g) Kc = 4.7 x 10-42
NO(g) + O3(g) ↔ NO2(g) + O2(g) Kc = 5.3 x 10-33
Based on this information, calculate Kc for the reaction: O2(g) + O(g) ↔ O3(g)
Expert's answer
NO(g) + O3(g) ↔ NO2(g) + O2(g)
Kc = 5.3 x 10-33
NO2(g) + O2(g) ↔ NO(g) + O3(g)
Kc1 = 5.3 x 10-33
NO2(g) ↔ NO(g) + O(g)
Kc = 4.7 x 10-42
NO(g) + O(g) ↔ NO2(g)
Kc2 = 4.7 x 10-42
Kc1 + Kc2 = Kc
Kc = -5.3 x 10-33 + -4.7 x 10-42 = -5.3 x 10-33
Kc = 5.3 x 10-33
NO2(g) + O2(g) ↔ NO(g) + O3(g)
Kc1 = 5.3 x 10-33
NO2(g) ↔ NO(g) + O(g)
Kc = 4.7 x 10-42
NO(g) + O(g) ↔ NO2(g)
Kc2 = 4.7 x 10-42
Kc1 + Kc2 = Kc
Kc = -5.3 x 10-33 + -4.7 x 10-42 = -5.3 x 10-33
