1.2046. 11:36 D A - O46 465 %A sample of pure NO2 isheated to 339 •C atwhich temperature itpartiallyaccordingequation : 2 NO2 (g)2NO (g) + O2 (g)dissociatestotheAtequilibrium,thedensitymixture is 0.520 g/L atofthegas0.755 atm. Calculate Kcfor the reaction.Kc = 0.133Kc = 1.35 x 10-4Kc = 0.0133||Kc = 0.045Continuebartlebu

A sample of pure NO2 is heated to 339 •C at which temperature it partially according equation : 2 NO2 (g) 2NO (g) + O2 (g) dissociates to the equilibrium, density mixture is 0.520 g/L at At the of the gas 0.755 atm. Calculate Kc for the reaction.

A sample of pure NO2 is heated to 339 •C at which temperature it partially according equation : 2 NO2 (g) 2NO (g) + O2 (g) dissociates to the equilibrium, density mixture is 0.520 g/L at At the of the gas 0.755 atm. Calculate Kc for the reaction.

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

1.20
46. 11:36 D A - O
46 46
5 %
A sample of pure NO2 is
heated to 339 •C at
which temperature it
partially
according
equation : 2 NO2 (g)
2NO (g) + O2 (g)
dissociates
to
the
At
equilibrium,
the
density
mixture is 0.520 g/L at
of
the
gas
0.755 atm. Calculate Kc
for the reaction.
Kc = 0.133
Kc = 1.35 x 10-4
Kc = 0.0133
||
Kc = 0.045
Continue
bartlebu

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