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4. At 2000°C the equilibrium constant for the reaction A(g) 2B(g) is Kp=1.0 x 105. If the initial partial pressure of A is 0.5 atm and the initial partial pressure of B is 1.0 atm, what are the equilibrium partial pressures of A and B?

4. At 2000°C the equilibrium constant for the reaction A(g) 2B(g) is Kp=1.0 x 105. If the initial partial pressure of A is 0.5 atm and the initial partial pressure of B is 1.0 atm, what are the equilibrium partial pressures of A and B?

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
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Can you please answer question 4
1. Given the equilibrium constant values at a certain temperature: 1/2N₂(g) + O₂(g)NO₂(g) Kp=1.0x 10-⁹ NOCI(g)+1/20₂(g) = NO₂Cl(g) Kp= 1.1 x 10² NO₂(g) +1/2Cl₂(g) = NO₂Cl(g) Kp = 0.30 Determine a value for Kp at this temperature for the reaction N₂ (g) +O₂(g) + Cl₂(g) 2NOC1 (g) 2. For the equilibrium at 1073K for 2H₂S(g) = 2H₂(g) + S₂(g), the Kp is 2.4 x 10-4. a. Calculate the Kc at this temperature. b. Calculate the Qp for this mixture: 0.112 atm H₂, 0.055 atm S₂, 0.455 atm H₂S. c. State in which direction this reaction mixture will proceed to reach equilibrium. 3. For the following reaction, Kc= 0.513 at 500 K. N₂O₂(g) = 2NO₂(g) If a reaction vessel initially contains an N₂O4 concentration of 0.0500M at 500 K, what are the equilibrium concentrations of N₂O4 and NO₂ at 500 K? 4. At 2000°C the equilibrium constant for the reaction A(g) 2B(g) is Kp=1.0 x 105. If the initial partial pressure of A is 0.5 atm and the initial partial pressure of B is 1.0 atm, what are the equilibrium partial pressures of A and B? 5. Consider the following endothermic reaction C₂H₂(g) + L₂(g) = C₂H₂L₂(g) If you were a chemist trying to maximize the amount of CHI(g) produced, which of the following would be appropriate to try? Select all that apply. a. Removing I(g) from the reaction mixture. b. The reaction mixture is heated c. Decreasing the reaction volume d. The total pressure of the system is increased by adding an inert noble gas. e. Adding CH (g) to the system.
Transcribed Image Text:1. Given the equilibrium constant values at a certain temperature: 1/2N₂(g) + O₂(g)NO₂(g) Kp=1.0x 10-⁹ NOCI(g)+1/20₂(g) = NO₂Cl(g) Kp= 1.1 x 10² NO₂(g) +1/2Cl₂(g) = NO₂Cl(g) Kp = 0.30 Determine a value for Kp at this temperature for the reaction N₂ (g) +O₂(g) + Cl₂(g) 2NOC1 (g) 2. For the equilibrium at 1073K for 2H₂S(g) = 2H₂(g) + S₂(g), the Kp is 2.4 x 10-4. a. Calculate the Kc at this temperature. b. Calculate the Qp for this mixture: 0.112 atm H₂, 0.055 atm S₂, 0.455 atm H₂S. c. State in which direction this reaction mixture will proceed to reach equilibrium. 3. For the following reaction, Kc= 0.513 at 500 K. N₂O₂(g) = 2NO₂(g) If a reaction vessel initially contains an N₂O4 concentration of 0.0500M at 500 K, what are the equilibrium concentrations of N₂O4 and NO₂ at 500 K? 4. At 2000°C the equilibrium constant for the reaction A(g) 2B(g) is Kp=1.0 x 105. If the initial partial pressure of A is 0.5 atm and the initial partial pressure of B is 1.0 atm, what are the equilibrium partial pressures of A and B? 5. Consider the following endothermic reaction C₂H₂(g) + L₂(g) = C₂H₂L₂(g) If you were a chemist trying to maximize the amount of CHI(g) produced, which of the following would be appropriate to try? Select all that apply. a. Removing I(g) from the reaction mixture. b. The reaction mixture is heated c. Decreasing the reaction volume d. The total pressure of the system is increased by adding an inert noble gas. e. Adding CH (g) to the system.
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