Nitrogen dioxide decomposes according to the reaction: 2 NO 2 (g) --> <-- 2 NO (

Question

                    Nitrogen dioxide decomposes according to the reaction:                                                       2 NO2 (g) --> <-- 2 NO (g) + O2(g)                                                       where Kp = 4.48 x 10-13 at a certain temperature.if 0.55 atm of NO2 is added to a container and allowedto come to equilibrium , what are                     the equilibrium partial pressuresof NO (g) and O2 (g)?                                      Nitrogen dioxide decomposes according to the reaction:                                      2 NO2 (g) --> <-- 2 NO (g) + O2(g)                                      where Kp = 4.48 x 10-13 at a certain temperature.if 0.55 atm of NO2 is added to a container and allowedto come to equilibrium , what are                     the equilibrium partial pressuresof NO (g) and O2 (g)?                 

Explanation / Answer

the equilibrium will shift to the right to produce more moles of gases,
in an attempt to restore the loss of pressure, according to LeChalelier's principle
2 NO2 <-----> 2NO + O2
initial pressure
0.55
at equilibrium
0.55 - 2x .. . . . 2x . .. . x

4.48*10-13 = 4x3 / 0.55-2x

4x3 = 0.55*4.48*10-13

x= 3.949 *10-5

equilibrium partial pressuresof NO (g) = 2*x = 7.898*10-5

O2 (g) =3.949 *10-5

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