15.23 The equilibrium constant for the reaction 2 NOBr (g) 2 NO(g) + Br2(g) 2 is K 1.3 x 10 at 1000 K. (a) At this temperature does the equilibrium favor NO and Br2, or does it favor NOBR? (b) Calculate K for 2 NOBr(g) = 2 NO(g ) + Br2(g). (c) Calculate K, for NOBr(g) NO (g) +Br2(g).

15.23 The equilibrium constant for the reaction 2 NOBr (g) 2 NO(g) + Br2(g) 2 is K 1.3 x 10 at 1000 K. (a) At this temperature does the equilibrium favor NO and Br2, or does it favor NOBR? (b) Calculate K for 2 NOBr(g) = 2 NO(g ) + Br2(g). (c) Calculate K, for NOBr(g) NO (g) +Br2(g).

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter13: Fundamental Equilibrium Concepts

Section: Chapter Questions

Problem 60E: At a temperature of 60 C, the vapor pressure of water is 0.196 atm. What is the value of the...

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Question

15.23 The equilibrium constant for the reaction
2 NOBr (g)
2 NO(g) + Br2(g)
2
is K 1.3 x 10 at 1000 K. (a) At this temperature does
the equilibrium favor NO and Br2, or does it favor NOBR?
(b) Calculate K for 2 NOBr(g) = 2 NO(g ) + Br2(g).
(c) Calculate K, for NOBr(g) NO (g) +Br2(g).

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