?Consider the equilibrium\(\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g)+\mathrm{Br}_{2}(g)

Chapter 15, Problem 15.28

(choose chapter or problem)

Consider the equilibrium

\(\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g)+\mathrm{Br}_{2}(g) \rightleftharpoons 2 \operatorname{NOBr}(g)\)

Calculate the equilibrium constant \(K_{p}\) for this reaction, given the following information (at 298 K):

\(2 \mathrm{NO}(g)+\mathrm{Br}_{2}(g) \rightleftharpoons 2 \mathrm{NOBr}(g) \quad K_{c}=2.0\)

\(2 \mathrm{NO}(g) \rightleftharpoons \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \quad K_{c}=2.1 \times 10^{30}\)

Text Transcription:

N2(g) + O2(g) + Br2(g) \rightleftharpoons 2 NOBr(g)

K_p

2 NO(g) + Br2(g) \rightleftharpoons 2 NOBr(g) Kc = 2.0

2 NO(g) \rightleftharpoons N2(g) + O2(g) Kc = 2.1 X 1030