The value of Kc for the reaction of dinitrogen tetroxide to make nitrogen dioxide is 2.3776. The concentration of nitrogen dioxide 1.4331 M with no dinitrogen tetroxide. What is the equilibrium concentration (in M) of nitrogen dioxide?
The equilibrium constant for the formation of nitrogen dioxide from dinitrogen tetraoxide is 2.3776.
i.e N2O4 <----------> 2NO2 Kc = 2.3776
For the backward reaction, we have ,
2NO2 <----------> N2O4 Kc = 0.4206
1 0
1.4331(1 - 2a) 1.4331a
0.4206 = (1.4331a) /[1.4331(1-2a)]2
1 + 4a2 - 4a = 1.659a
1+ 4a2 - 5.659a = 0
by solving we get :-
a = 0.2069 and a= 1.2077
by neglecting a = 1.2077 we get
a = 0.2069
equilibrium concentration of nitrogendioxide = 1.4331( 1- 0.4138) = 0.8400 M
equilibrium concentration of dinitrogen tetraoxide = 0.2965
The value of Kc for the reaction of dinitrogen tetroxide to make nitrogen dioxide is 2.3776....
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