3. In a 2.000-Liter vessel at 226 °C, a mixture of 0.2000 mol of CO2, 0.1000 mol of H₂ and 0.1600 mol of H₂O is placed. The following equilibrium is established given the chemical equation: CO2(g) + H₂(g) CO(g) + H₂O(g). a. Calculate the initial partial pressures of CO2, H2 and H₂O. b. At equilibrium, calculate the equilibrium partial pressures of CO2, H2 and Co. c. Calculate Kp for the reaction. H

3. In a 2.000-Liter vessel at 226 °C, a mixture of 0.2000 mol of CO2, 0.1000 mol of H₂ and 0.1600 mol of H₂O is placed. The following equilibrium is established given the chemical equation: CO2(g) + H₂(g) CO(g) + H₂O(g). a. Calculate the initial partial pressures of CO2, H2 and H₂O. b. At equilibrium, calculate the equilibrium partial pressures of CO2, H2 and Co. c. Calculate Kp for the reaction. H

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

Section: Chapter Questions

Problem 97QRT

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A solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent CCl4.The total solution volume is 1.00 L When the reaction C6H10I2 C6H10 + I2 has come to equilibrium at 35 C, the concentration of I2 is 0.035 mol/L. (a) What are the concentrations of C6H10I2 and C6H10 at equilibrium? (b) Calculate Kc, the equilibrium constant.
Consider 0.200 mol phosphorus pentachloride sealed in a 2.0-L container at 620 K. The equilibrium constant, Kc, is 0.60 for PCl5(g) PCl3(g) + Cl2(g) Calculate the concentrations of all species after equilibrium has been reached.
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