Consider the equilibrium: 2N20(g) + O2(g)=4NO(g)3.00 moles of NO(g) are introduced into a 1.00-Liter evacuated flask. When the systemequilibrium,1.00 mole of N20(g) has formed. Determine the equilibrium concentrations of eachsubstance. Calculate the Kc for the reaction based on these data.comes to2 N20O24 NOinitialchangeequilibriumRemember: The "ice" box may be used with moles, molarity, or Liters (for gaseous equilibria)...never grams.

volume of the flask is 1L Initially,[NO] = 3 mol/1L = 3M At equilibrium,[N2O]=1M

Consider the equilibrium: 2N2O(g) + O2(g)=4NO(g) 3.00 moles of NO(g) are introduced into a 1.00-Liter evacuated flask. When the system quilibrium,1.00 mole of N20(g) has formed. Determine the equilibrium concentrations of each ubstance. Calculate the Kc for the reaction based on these data. comes to 2 N2O O2 4 NO initial change equilibrium

Consider the equilibrium: 2N2O(g) + O2(g)=4NO(g) 3.00 moles of NO(g) are introduced into a 1.00-Liter evacuated flask. When the system quilibrium,1.00 mole of N20(g) has formed. Determine the equilibrium concentrations of each ubstance. Calculate the Kc for the reaction based on these data. comes to 2 N2O O2 4 NO initial change equilibrium

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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