Given the equilibrium reaction: H₂C₂O₄ ⇌ 2H⁺ + C₂O₄²⁻, calculate the equilibrium concentration of C₂O₄²⁻ in a 0.20 M solution of oxalic acid, assuming the acid dissociates completely. The equilibrium constant, Kₐ, for the first dissociation is 5.5 x 10⁻².

An equilibrium mixture of CO, O2, and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0020 M O2. At this temperature, Kc equals 1.4 × 10^2 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g). What is the equilibrium concentration of CO?

At a certain temperature, the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICl(g) ⇌ I2(g) + Cl2(g). What is the equilibrium concentration of ICl if 0.45 mol of I2 and 0.45 mol of Cl2 are initially mixed in a 2.0-L flask?

What is the equilibrium constant expression for a reaction at equilibrium?

Calculate the equilibrium constant (K) for the reaction: 2 N2O (g) + 3 O2 (g) ⇌ 2 N2O4 (g), using the following information: 1) 2 N2 (g) + O2 (g) ⇌ 2 N2O (g) K1 = 1.2 x 10^-35 2) N2O4 (g) ⇌ 2 NO2 (g) K2 = 4.6 x 10^-3 3) ½ N2 (g) + O2 (g) ⇌ NO2 (g) K3 = 4.1 x 10^-9

Given the reaction Fe²⁺(aq) + Mn(s) ⇌ Fe(s) + Mn²⁺(aq), calculate the equilibrium constant (K) at 25°C if the concentrations at equilibrium are [Fe²⁺] = 0.010 M and [Mn²⁺] = 0.020 M. Express your answer to two significant figures.

Consider the following reaction: 2CH4(g) ⇌ C2H2(g) + 3H2(g). The reaction of CH4 is carried out at some temperature with an initial concentration of [CH4] = 0.089 M. At equilibrium, the concentration of H2 is 0.010 M. Find the equilibrium constant (Kc) for the reaction.

Consider the following reaction: SO2Cl2(g) ⇌ SO2(g) + Cl2(g). Kc = 2.99×10⁻⁷ at 227 °C. If a reaction mixture initially contains 0.150 M SO2Cl2, what is the equilibrium concentration of Cl2 at 227 °C?

Consider the following reaction: CH4(g) + 2 H2S(g) ⇌ CS2(g) + 4 H2(g). A reaction mixture initially contains 0.50 M CH4 and 0.75 M H2S. If the equilibrium concentration of H2 is 0.44 M, find the equilibrium constant (Kc) for the reaction.