?The equilibrium constant for the reaction\(2 \mathrm{NO}(g)+\mathrm{Br}_{2}(g)

Chapter 15, Problem 15.23

(choose chapter or problem)

The equilibrium constant for the reaction

\(2 \mathrm{NO}(g)+\mathrm{Br}_{2}(g) \rightleftharpoons 2 \operatorname{NOBr}(g)\)

is \(K_{c}=1.3 \times 10^{-2}\) at 1000 K.

(a) At this temperature does the equilibrium favor \(\mathrm{NO}\) and \(\mathrm{Br}_{2}\), or does it favor NOBr?

(b) Calculate \(K_{c}\) for \(2 \operatorname{NOBr}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{Br}_{2}(g)\).

(c) Calculate \(K_{c}\) for \(\operatorname{NOBr}(g) \rightleftharpoons \mathrm{NO}(g)+\frac{1}{2} \mathrm{Br}_{2}(g)\).

Text Transcription:

2 NO(g) + Br2(g) \rightleftharpoons 2 NOBr(g)

K_c = 1.3 X 10-2

Br_2

K_c

2 NOBr(g) \rightleftharpoons 2 NO(g) + Br2(g)

NOBr(g) \rightleftharpoons NO(g) + 1 2 Br2(g)