Consider the following reaction: 2 H2O(g) + 2 SO2(g) ⇌ 2 H2S(g) + 3 O2(g). A reaction mixture initially contains 2.8 M H2O and 2.6 M SO2. Determine the equilibrium concentration of H2S if Kc for the reaction at this temperature is 1.3 × 10^-6.

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.

Consider the following reaction: 2 H2O(g) + 2 SO2(g) <--> 2 H2S(g) + 3 O2(g). A reaction mixture initially contains 2.8 M H2O and 2.6 M SO2. Determine the equilibrium concentration of H2S if Kc for the reaction at this temperature is 1.3 x 10^-6.

Consider the reaction C2H4(g) + H2O(g) -> CH3CH2OH(g). Using the standard thermodynamic data, calculate the equilibrium constant (K) for this reaction at 298.15 K.

Consider the reaction: H2(g) + I2(g) ⇌ 2HI(g). A reaction mixture in a 3.730-L flask at a certain temperature initially contains 0.7660 g H2 and 97.10 g I2. At equilibrium, the flask contains 90.40 g HI. Calculate the equilibrium constant (Kc) for the reaction.

Consider the reaction, which takes place at a certain elevated temperature: CO(g) + NH3(g) ⇌ HCONH2(g), Kc = 0.690. If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00 M and 2.00 M, respectively, what will be the concentration of HCONH2(g) at equilibrium?