Reversible Reactions and Equilibrium Quiz

Consider the reaction. N2(g) + 3H2(g) <--> 2NH3(g) At equilibrium, the concentrations of the different species are as follows. [NH3] = 0.105 M [N2] = 1.1 M [H2] = 1.50 M What is the equilibrium constant for the reaction at this temperature?

0.0030

Consider the reaction. 2NOCl(g) <--> 2NO(g) + Cl2(g) At equilibrium, the concentrations are as follows. [NOCl] = 1.4 ´ 10-2 M [NO] = 1.2 ´ 10-3 M [Cl2] = 2.2 ´ 10-3 M What is the value of Keq for the reaction expressed in scientific notation?

1.6 ´ 10-5

Consider the reaction. 2HF(g) <--> H2(g) + F2(g) At equilibrium at 600 K, the concentrations are as follows. [HF] = 5.82 x 10-2 M [H2] = 8.4 x 10-3 M [F2] = 8.4 x 10-3 M What is the value of Keq for the reaction expressed in scientific notation?

2.1 x 10-2

Which statement correctly defines dynamic equilibrium?

At dynamic equilibrium, the rates of forward and reverse reactions are equal.

Which statement correctly describes a reaction in dynamic equilibrium?

At dynamic equilibrium, the reactions continue but the amounts of reactants and products do not change.

Consider the general reversible reaction. aA + bB <--> cC + dD What is the equilibrium constant expression for the given system?

Keq = [C]c[D]d/[A]a[B]b

Which represents the correct equilibrium constant expression for the reaction below? Cu(s) + 2Ag+(aq) <--> Cu2+(aq) + 2Ag(s)

Keq = [Cu2+]/[ag+]^2

Consider the following reversible reaction. 2H2O(g) <--> 2H2(g) + O2(g) What is the equilibrium constant expression for the given system?

Keq = [H2]^2[O2]/[H2O]^2

Consider the reaction below. 2N2O5(g) <--> 4NO2(g) + O2(g) If the reaction is at dynamic equilibrium at 500 K, which statement applies to the given chemical system?

The concentrations of the products and reactants do not change.

The reaction below is at dynamic equilibrium. N2(g) + 3H2 <--> 2NH3(g) Which statement is true for the equilibrium system?

The rate of the forward reaction equals the rate of the reverse reaction.