16.6 (Pages 696 - 699); Watch IWE 16.5. Consider the following reaction: CO (g) + 2 H₂ (g) = CH3OH (g) A reaction mixture in a 5.25-L flask at a certain temperature initially contains 27.1 g CO and 2.36 g H₂. At equilibrium, the flask contains 8.67 g CH3OH. Calculate the equilibrium constant (Kc) for the reaction at this temperature. ► View Available Hint(s) Kc = {—| ΑΣΦ ?

Suppose a 500. mL flask is filled with 0.30 mol of Br,, 1.5 mol of OCl, and 1.0 mol of BrOCl. The following reaction becomes possible: Br, (g) +OCl, (g) – BROC1(g) +BrC1(g) The equilibrium constant K for this reaction is 0.214 at the temperature of the flask. Calculate the equilibrium molarity of BrOCl. Round your answer to two decimal places. do Ar OM ?

At a certain temperature, the equilibrium constant K for the following reaction is 6.0 x 10: co(e) + H,0(g) -co,() + H,(g) Use this information to complete the following table. Suppose a 31. L reaction vessel is filled with 1.1 mol of co, and 1.1 mol of H2. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little CO and H,0. O There will be very little Co, and H,. O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = ] Co,(0)+H,(0) CO()+H,O(9) 1. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = ] 3 CO0g)+3H,0(9) 3 CO,(0)+3H,(9) 1.

Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 2.0 L flask with 4.7 atm of sulfur dioxide gas and 0.67 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 0.80 atm. Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K = 0 P 0 x10