Consider the following reactions and their respective equilibrium constants: NO(g) + Br₂(g) NOBr(g); K = 5.3 2NO(g) = N₂(g) + O₂(g); K= 2.1 × 10³0 Use these reactions and their equilibrium constants to predict the equilibrium constant for the following reaction: N₂(g) + O₂(g) + Br2(g) = 2NOBr(g) Express your answer using two significant figures.

Consider the following reactions and their respective equilibrium constants: NO(g) + Br₂(g) NOBr(g); K = 5.3 2NO(g) = N₂(g) + O₂(g); K= 2.1 × 10³0 Use these reactions and their equilibrium constants to predict the equilibrium constant for the following reaction: N₂(g) + O₂(g) + Br2(g) = 2NOBr(g) Express your answer using two significant figures.

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 38A

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