16. Chemical Equilibrium

How can the reverse equilibrium constant for the reaction 8 H₂(g) + 8 Br₂(g) ⇌ 16 HBr(g) be expressed?

Calculate the equilibrium constant Kc for the reaction N2O4(g) ⇌ 2NO2(g) given that at equilibrium at 100°C, [N2O4] = 0.0014 M and [NO2] = 0.0172 M.

For the reaction A ⇌ B at equilibrium, if the concentration of A is 0.5 M and the concentration of B is 2.0 M, what is the value of the equilibrium constant Kc?

What is the equilibrium constant expression (K) for the reaction: CO2(g) + C(s) ⇌ 2 CO(g)?

For the reaction N_2(g) + 3H_2(g) ightleftharpoons 2NH_3(g), the equilibrium concentrations at a certain temperature are [N_2] = 0.50 M, [H_2] = 1.50 M, and [NH_3] = 2.00 M. What is the value of the equilibrium constant K_c for this reaction?

What is the equilibrium constant expression (K) for the reaction: 2 H_2(g) + O_2(g) ightleftharpoons 2 H_2O(g)?

For the reaction N_2(g) + 3H_2(g) ightarrow 2NH_3(g), the equilibrium concentrations at 500 K are [N_2] = 0.20 M, [H_2] = 0.60 M, and [NH_3] = 1.2 M. What is the value of the equilibrium constant K_c for this reaction in correct scientific notation?

Given the reaction N_2(g) + 3H_2(g) ightarrow 2NH_3(g), and the following equilibrium concentrations obtained from a graph: [N_2] = 0.20 M, [H_2] = 0.60 M, [NH_3] = 1.20 M, estimate the value of the equilibrium constant K_c for this reaction.

Given the reaction: N_2(g) + 3H_2(g) ightleftharpoons 2NH_3(g), the equilibrium constant K for this reaction is:

Given the reaction: FeCl_3(aq) + 3NH_4SCN(aq) ⇌ Fe(SCN)_3(aq) + 3NH_4Cl(aq), which of the following is the correct equilibrium constant expression (K) for this reaction?

For the reaction 2 R (g) ⇌ Q (g), if the equilibrium concentration of R is 0.776 M and that of Q is 1.22 M at 25 °C, what is the value of the equilibrium constant K at this temperature?

Which values of the equilibrium constant K indicate that there is more product B than reactant A at equilibrium for the reaction A ⇌ B?

What is the equilibrium constant expression (K) for the reaction: CO2(g) + H2(g) ⇌ CO(g) + H2O(l)?

For the following aqueous reaction at 298 K: N2(g) + 3 H2(g) ⇌ 2 NH3(g), what is the value of the equilibrium constant K if the equilibrium concentrations are [N2] = 0.20 M, [H2] = 0.30 M, and [NH3] = 0.40 M?

What does a very small equilibrium constant (K << 1) indicate about a chemical reaction at equilibrium?