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

n2(g) + 3h2-> 2nh3(g)   this is the balanced equation

note the mole ratio between n2, h2 and nh3.   it is 1 : 3 : 2   this will be important.

moles n2 present = 28.0 g n2 x 1 mole n2/28 g = 1 mole n2 present

moles h2 present = 25.0 g h2 x 1 mole h2/2 g = 12.5 moles h2 present

based on mole ratio, n2 is limiting in this situation because there is more than enough h2 but not enough n2.

moles nh3 that can be produced = 1 mole n2 x 2 moles nh3/mole n2 = 2 moles nh3 can be produced

grams of nh3 that can be produced = 2 moles nh3 x 17 g/mole = 34 grams of nh3 can be produced

note:   the key to this problem is recognizing that n2 is limiting, and therefore limits how much nh3 can be produced.

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