16. Chemical Equilibrium

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: 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?

Estimate the value of the equilibrium constant (K) at 660 K for the reaction 2NO2(g) ⇌ N2O4(g), given that ΔG°f for BrCl(g) is -1.0 kJ/mol, the standard molar entropy S° for BrCl(g) is 240.0 J/mol·K, and ΔH°f for N2O4(g) is 9.16 kJ/mol.

Given that Kc is 1.67 × 10^20 at 25°C for the formation of the iron(III) oxalate complex ion: Fe3+(aq) + 3 C2O4^2-(aq) ⇌ [Fe(C2O4)3]^3-(aq), and 0.0200 M Fe3+ is initially mixed with 1.00 M oxalate ion, what is the concentration of Fe3+ ion at equilibrium?

A solution initially contains [Ag+] of 3.2 × 10^-3 M and 0.125 M NH3. What is the concentration of Ag+ after the solution reaches equilibrium, given that the formation constant (Kf) of Ag(NH3)2+ is 1.7 × 10^7?

Given the reaction 2COF2(g) ⇌ CO2(g) + CF4(g) with an equilibrium constant Kp = 2.2 × 10^6 at 298 K, what is the equilibrium constant Kp for the reaction 4COF2(g) ⇌ 2CO2(g) + 2CF4(g)?

For the reaction CO (g) + Cl2 (g) ⇌ COCl2 (g) with Kc = 255 at 1000 K, a reaction mixture initially contains a CO concentration of 0.1510 M and a Cl2 concentration of 0.175 M at 1000 K. What is the equilibrium concentration of COCl2?

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.

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

At a certain temperature, Kc equals 1.4 × 10^2 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g). If a 2.50-L flask contains 0.400 mol of CO2 and 0.100 mol of O2 at equilibrium, how many moles of CO are also present in the flask?

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.

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