The reaction. N₂0₁2 NO₂ is allowed to reach equilibrium in a chloroform solution at 25 °C. The equilibrium concentrations are 0.490 mol/L N₂O, and 2.34 mol/L NO₂. Calculate the equilibrium constant, K., for this reaction. K₂ = 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 NO, is added. O towards the reactant towards the product no change Determine how the addition of extra NO, in the previous step will affect the rate constant, K. Ke will increase Ke will decrease Ke will not change
The reaction. N₂0₁2 NO₂ is allowed to reach equilibrium in a chloroform solution at 25 °C. The equilibrium concentrations are 0.490 mol/L N₂O, and 2.34 mol/L NO₂. Calculate the equilibrium constant, K., for this reaction. K₂ = 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 NO, is added. O towards the reactant towards the product no change Determine how the addition of extra NO, in the previous step will affect the rate constant, K. Ke will increase Ke will decrease Ke will not change
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
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 23Q: Consider the reaction 2N2O(g) + O2(g) 4NO(g) Suppose the system is at equilibrium, and then an...
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