For the equilibrium reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g), the equilibrium constant Kc at a certain temperature is 0.5. If the initial concentrations of N₂ and H₂ are both 1.0 M, what will be the equilibrium concentration of NH₃?

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?

For the combustion reaction 2H₂(g) + O₂(g) → 2H₂O(g), what is the likely magnitude of the equilibrium constant K at a given temperature?

If Kc = 0.600 and Kp = 359 for a hypothetical reaction, which of the following equations could represent the reaction at 25°C?

The Keq for the equilibrium below is 5.4 x 10^13 at 480.0°C.2NO (g) + O2 (g) ↔ 2NO2 (g)What is the value of Keq at this temperature for the following reaction?NO (g) + 1/2 O2 (g) ↔ NO2 (g)

What is the equilibrium constant expression for the reaction 2 SO3(g) ⇌ 2 SO2(g) + O2(g)?

What is the expression for the equilibrium constant (K) for the reaction: Li(s) + 2H2O(l) ⇌ Li+(aq) + 2OH-(aq) + H2(g)?

What is the approximate value of the equilibrium constant, Kₙ, for the neutralization of hydrochloric acid with sodium hydroxide, shown in the equation below? HCl(aq) + NaOH(aq) → H₂O(l) + NaCl(aq)