Question

The equilibrium between ozone and dioxygen is represented by: 2O3 (g) ⇌ 3O2 (g) Kc = 2.5 × 10^15 at 273 K. Calculate the molarity of ozone in an atmospheric sample of air that has an O2 concentration of 0.0089 M (0.2 moles in 22.4 L) at STP. ANS = 1.7 × 10^-11 If the equilibrium constant for the reaction: N2(g) + O2(g) ⇌ 2NO(g) is 4.8 × 10^-31, what is the equilibrium constant for the reaction: 2NO(g) ⇌ N2(g) + O2(g)? ANS = 2.1 × 10^30

Name: a the equilibrium between ozone and dioxygen is represented by 2o3 g 3o2 g kc 25 1015 at 273 k calculate the molarity of ozone in an atmospheric sample of air that has an o2 concentration of 57033
Uploaded: 2022-02-20T16:16:34-08:00
Duration: 1 min 5 s
Channel: Dinesh Singh
Description: a the equilibrium between ozone and dioxygen is represented by 2o3 g 3o2 g kc 25 1015 at 273 k calculate the molarity of ozone in an atmospheric sample of air that has an o2 concentration of 57033

          The equilibrium between ozone and dioxygen is represented by: 2O3 (g) ⇌ 3O2 (g) Kc = 2.5 × 10^15 at 273 K. Calculate the molarity of ozone in an atmospheric sample of air that has an O2 concentration of 0.0089 M (0.2 moles in 22.4 L) at STP.
ANS = 1.7 × 10^-11

If the equilibrium constant for the reaction: N2(g) + O2(g) ⇌ 2NO(g) is 4.8 × 10^-31, what is the equilibrium constant for the reaction: 2NO(g) ⇌ N2(g) + O2(g)?
ANS = 2.1 × 10^30

Added by Melvin B.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Dinesh Singh

02/20/2022

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5 × 10^15 N2(g) + O2(g) ⇌ 2NO(g) Kc = 4.8 × 10^-31 Show more…

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The equilibrium between ozone and dioxygen is represented by: 2O3 (g) ⇌ 3O2 (g) Kc = 2.5 × 10^15 at 273 K. Calculate the molarity of ozone in an atmospheric sample of air that has an O2 concentration of 0.0089 M (0.2 moles in 22.4 L) at STP. ANS = 1.7 × 10^-11 If the equilibrium constant for the reaction: N2(g) + O2(g) ⇌ 2NO(g) is 4.8 × 10^-31, what is the equilibrium constant for the reaction: 2NO(g) ⇌ N2(g) + O2(g)? ANS = 2.1 × 10^30