Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.79 at a certain temperature. If a reaction mixture initially contains 0.050 M H2S and 0.050 M SO2, what will the equilibrium concentration of H2O be? 2 H2S(g) + SO2(g) = 3 S(s) + 2 H;O(g)

Calculating an equilibrium constant from a partial equilibrium composition Steam reforming of methane ( CH4 ) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 1.5 L flask with 4.3 atm of methane gas and 1.8 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 3.2 atm. Calculate the pressure equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K p 11] ☐ x10 ☑ ⑤

Part A The equilibrium constant, Kc, for the decomposition of COC2 to CO and Cl2 is 0.68. If an equilibrium mixture contains 0.38 M CÓ and 0.55 M Cl2, what is the molar concentration of COCl2 ? COC2 (g) = CO(g) + Cl2 (g) Express your answer to two significant figures and include the appropriate units.

Suppose a 250. mL flask is filled with 0.40 mol of H₂ and 1.3 mol of HI. This reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of H₂. You can leave out the M symbol for molarity. initial cha equilibrium H₂ 0 X 0 1₂ 0 HI 00 믐 X olo 18 Ar