Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO2(g). N2O4(g) ↔ 2 NO2(g) Kc = 0.21 [N2O4]eq = 0.033 M

Thus, the equilibrium concentration of is 0.083 M

Explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as

Molarity of   at equilibrium = 0.033 M

The given balanced equilibrium reaction is,

  At eqm. conc.     (0.033) M           x 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 = 0.083 M

Thus, the concentrations of at equilibrium is 0.083 M

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.