The reaction below is carried out at a different temperature at which Kc=0.055. This time, however, the reaction mixture starts with only the product, [NO]=0.0100M, and no reactants. Find the equilibrium concentrations of N2, O2, and NO at equilibrium.

Thee given question is incomplete. the complete question is:

The reaction below is carried out at a different temperature at which Kc = 0.055. This time, however, the reaction mixture starts with only the product, [NO] = 0.0100 M, and no reactants. Find the equilibrium concentrations of N2, O2, and NO at equilibrium. The equation is N2(g) + O2(g) <--> 2NO(g)

Concentration of at equilibrium = 0.001 M

Concentration of = 0.0045 M

Concentration of  = 0.0045 M

Explanation:

Equilibrium constant is the ratio of the concentration of products to the concentration of reactants each term raised to its stoichiometric coefficients.

Initial concentration of = 0.0100 M

The given balanced equilibrium reaction is,

Initial conc.            0 M           0 M         0.0100 M

At eqm. conc.     (x) M          (x) M       (0.0100-2x) M

The expression for equilibrium constant for this reaction will be,

Now put all the given values in this expression, we get :

By solving the term 'x', we get :

x = 0.0045

Thus, the concentrations of at equilibrium are :

Concentration of at equilibrium = (0.0100-2x) M  =

Concentration of = (x) M = 0.0045 M

Concentration of = (x) M = 0.0045 M

a non redox reaction occurs when there is not a transfer of electrons. for redox reactions, which are reduction-oxidation reactions, a change in the oxidation number occurs. elements that are reduced gain electrons, and elements that are oxidized lose electrons.

explanation:

"the periodic table is arranged in order of atomic number."