The reaction N₂O₁ = 2NO₂ N204 is allowed to reach equilibrium in a chloroform solution at 25 °C. The equilibrium concentrations are 0.443 mol/L N2O4 and 2.23 mol/L. NO,. Calculate the equilibrium constant, Ke, for this reaction. KC = 11.2 An additional 1.00 mol NO₂ is added to 1.00 L of the solution and the system is allowed to reach equilibrium again at the same temperature. Select the direction of the equilibrium shift after the NO2 is added. no change towards the product towards the reactant Determine how the addition of extra NO2 in the previous step will affect the rate constant, Kc. Ke will decrease OK, will not change Ke will increase Calculate the equilibrium concentrations of N2O4 and NO2 after the extra 1.00 mol NO2 is added to 1.00 L of solution. [N,O₁] = [NO₂] = TOOLS x10 mol/L mol/L

The reaction N₂O₁ = 2NO₂ N204 is allowed to reach equilibrium in a chloroform solution at 25 °C. The equilibrium concentrations are 0.443 mol/L N2O4 and 2.23 mol/L. NO,. Calculate the equilibrium constant, Ke, for this reaction. KC = 11.2 An additional 1.00 mol NO₂ is added to 1.00 L of the solution and the system is allowed to reach equilibrium again at the same temperature. Select the direction of the equilibrium shift after the NO2 is added. no change towards the product towards the reactant Determine how the addition of extra NO2 in the previous step will affect the rate constant, Kc. Ke will decrease OK, will not change Ke will increase Calculate the equilibrium concentrations of N2O4 and NO2 after the extra 1.00 mol NO2 is added to 1.00 L of solution. [N,O₁] = [NO₂] = TOOLS x10 mol/L mol/L

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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