Use the References to access important values if needed for this question. The equilibrium constant, Kp, for the following reaction is 10.5 at 350. K. 2CH₂Cl2 (9) ⇒ CH4 (9) + CCl4 (9) If an equilibrium mixture of the three gases in a 12.5 L container at 350. K contains CH₂Cl₂ at a pressure of 0.276 atm and CH4 at a pressure of 0.593 atm, the equilibrium partial pressure of CCl4 is atm. Submit Answer Retry Entire Group 8 more group attempts remaining

Methanol liquid burns readily in air. One way to represent this equilibrium is: 2 CH3ОН(1) + 3 02(9)+ 2 CO2(g) + 4 H20(g) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1) CНH3ОН(1) + 3/2 02(9)+ =cO2(g) + 2 H20(g) K1 = %D 2) 2 CO2(9) + 4 H20(g) 2 CH3ОН (1) + 3 02(9) K2 = 3) СO2(g) + 2 H20(g) еснзон (1) + 3/2 02(g) K3 : %3D Drag and drop your selection from the following list to complete the answer: к1/2 1/K (1/K)!/2

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 500. mL flask is filled with 0.20 mol of NO, and 1.3 mol of NO. This reaction becomes possible: 2NO,(g) = 2NO(g)+0,(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 O,. You can leave out the M symbol for molarity. NO, NO 0, initial ? change equilibrium

12) If 1.34 moles each of Br2 and Cl2 are introduced into an 11.0 liter flask and allowed to come to equilibrium, what should the equilibrium concentrations of Br2, Cl2, and BrCl be? 2 BrCl (g) « Br2 (g) + Cl2 (g)​​​Kc = 0.143

Suppose a 500. mL flask is filled with 0.70 mol of Br,, 1.8 mol of BrOCl and 1.1 mol of BrCl. The following reaction becomes possible: Br, (g) + OCl,(g) =BROC1 (g)+BrCl (g) The equilibrium constant K for this reaction is 0.244 at the temperature of the flask. Calculate the equilibrium molarity of BrOCI. Round your answer to two decimal places. ?

3. If the equilibrium constant K, for the reaction 2 NO (g) + O2(g) = 2 NO2 (g) is 5.0 x 1012 at a given temperature, what is the value of the equilibrium constant K, for each of the following reactions at the same temperature? a) NO (g) + ½ O2 (g) → NO2 (g) b) 2 NO2 (g) = 2 NO (g) + 02 (g) c) NO2(g) = NO (g) + ½ 02 (g)

Consider the following reaction: 2NOBr(g) 2NO(g) + Br₂ (9) for this question. If 0.340 moles of NOBr(g), 0.327 moles of NO, and 0.499 moles of Br₂ are at equilibrium in a 12.3 L container at 445 K, the value of the equilibrium constant, Ke, is

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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