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.

At T = 700 K, the equilibrium constant for the reaction CCl4(g) ⇌ C(s) + 2 Cl2(g) is K_p = 0.76. A flask is charged with 3.0 atm of CCl4(g) at 700 K, which is then allowed to reach equilibrium. What is the partial pressure of Cl2(g) in the flask?

At a certain temperature, the equilibrium constant Kc for the reaction 2 C(s) + O2(g) ⇌ 2 CO(g) is 4.72. What is the equilibrium constant Kc for the reverse reaction CO(g) ⇌ C(s) + 0.5 O2(g) at the same temperature?

Calculate the equilibrium constant Kc at 256 K for the reaction SO2(g) + Cl2(g) ⇌ SO2Cl2(g) if Kp = 42 at this temperature. Assume the reaction involves gases and use the relation between Kp and Kc.

Calculate the equilibrium constant Kc at 304 K for the reaction SO2(g) + Cl2(g) ⇌ SO2Cl2(g) if the equilibrium constant Kp is 33.0 at this temperature.

Consider the following equilibrium, for which Kp = 7.54×10⁻² at 490 °C: 2Cl2(g) + 2H2O(g) ⇌ 4HCl(g) + O2(g). What is the value of Kc for the following reaction? Cl2(g) + H2O(g) ⇌ 2HCl(g) + 0.5O2(g)

Consider the reaction: 2CO(g) + O2(g) ⇌ 2CO2(g). What is the correct equilibrium expression for this reaction?

Consider the reaction: A2 + B2 <--> 2AB. The reactants are mixed together, and the following is a plot of the reactant and the product concentrations with time. If at equilibrium, the concentration of A2 is 0.5 M, B2 is 0.5 M, and AB is 1.0 M, what is the value of the equilibrium constant K?

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?