Question

Can anyone tell me how to solve this what steps do i take..

Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide?
3N₂O₄(g)  6NO₂ (g)

[A] [N₂O₄] ⁶ /[NO₂] ³                  [B] [NO₂] ⁶ /[N₂O₄] ³  

[C] [NO₂] ³ /[N₂O₄] ³                  [D] [N₂O₄] ³ /[NO₂] ³               [E] [NO₂] ³ /[N₂O₄] ⁶

Answer 1

first write the balanced equation

3N₂O₄ (g) -------> 6NO₂ (g)

now you reed the definition of equilibrium constant definetely

Equilibrium Constant Definition: The equilibrium constant is the ratio of the equilibrium concentrations of the products raised to the power of their stoichiometric coefficients to the equilibrium concentrations of the reactants raised to the power of their stoichiometric coefficients.

in you r reaction product is NO2 and its stoichiomtry coefficient is 6 ok

in your reaction product is N2O4 and and its stoichiometric coefficient is 3

now Kc = [NO2] ⁶ / [N2O4] ³ is the answer

i hope you got it