At a unspecified temperature we place 0.940 mol of pure SO3 is placed in a evacuated 1.00-L container, and the following reaction occurs 2 SO3(g) 2 SO₂(g) + O₂(g) At equilibrium we find 0.190 mol of O₂ is present. Determine the value for the equilibrium constant in terms of concentrations. Kc =

Suppose a 500. mL flask is filled with 0.80 mol of NO and 1.8 mol of NO2. The following reaction becomes possible: NO3(g) + NO(g) - 2NO2(g) The equilibrium constant K for this reaction is 4.37 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places.

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 5.0 L flask with 4.3 atm of sulfur dioxide gas and 3.9 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 3.9 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

Suppose a 250. mL flask is filled with 0.80 mol of O2 and 0.30 mol of SO3. This reaction becomes possible: 2SO2(g) + O2(g) ~ 2SO3(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 r to stand for the unknown change in the molarity of O,. You can leave out the M symbol for molarity.

Suppose a 500. mL flask is filled with 1.9 mol of N, and 0.20 mol of NO. The following reaction becomes possible: N₂(g) + O₂(g) → 2NO(g) The equilibrium constant K for this reaction is 3.27 at the temperature of the flask. Calculate the equilibrium molarity of N₂. Round your answer to two decimal places.

Calculating equilibrium composition from an equilibrium constant Suppose a 250, mil. flask is filled with 1.5 mol of NO₂, 0.10 mol of CO and 2.0 mol of CO₂. The following reaction becomes possible: NO₂(g) +CO(g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 0.226 at the temperature of the flask. Calculate the equilibrium molarity of NO₂. Round your answer to two decimal places. OM Explanation CIU Check DEC 9 X 3 6 tv 8

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 500. mL flask with 1.2 atm of sulfur dioxide gas and 4.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 0.60 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 x10 5

Suppose a 250. mL flask is filled with 1.8 mol of O2 and 0.30 mol of NO. The following reaction becomes possible: N₂(g) + O₂(g) → 2NO(g) The equilibrium constant K for this reaction is 2.61 at the temperature of the flask. Calculate the equilibrium molarity of O2. Round your answer to two decimal places. M X S

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 1.5 L flask with 1.7 atm of sulfur dioxide gas and 4.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 1.0 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 = [|

Suppose a 250. mL flask is filled with 1.2 mol of H₂ and 0.90 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 I2. You can leave out the M symbol for molarity. H₂ 1₂ HI initial 1.2 0 ? change X equilibrium