The equilibrium constant, K, for the following reaction is 55.6 at 698 K.H2 (g) + I2 (g)= 2 HI (g)Calculate the equilibrium concentrations of reactants and product when 0.205moles of H2 and 0.205 moles of I, are introduced into a 1.00 L vessel at 698 K.[H2] =|M[1 ]M%3D[ HI ] =M Consider the following system at equilibrium where AH = -198 kJ, and K. = 34.5, at 1.15×10° K.2502(g) + 02(g)=2503(g)If the VOLUME of the equilibrium system is suddenly increased at constant temperature:The value of K.]A. increases.B. decreases.C. remains the same.A. is greater than K..B. is equal to KeC. is less than K.The value of Qe|A. run in the forward direction to reestablish equilibrium.The reaction must:B. run in the reverse direction to reestablish equilibrium.C. remain the same. It is already at equilibrium.The number of moles of O, will:A. increase.B. decrease.C. remain the same.

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The equilibrium constant, Ke, for the following reaction is 55.6 at 698 K. H2 (g) + I2 (g)=2 HI (g) Calculate the equilibrium concentrations of reactants and product when 0.205 moles of H2 and 0.205 moles of I, are introduced into a 1.00 L vessel at 698 K.

The equilibrium constant, Ke, for the following reaction is 55.6 at 698 K. H2 (g) + I2 (g)=2 HI (g) Calculate the equilibrium concentrations of reactants and product when 0.205 moles of H2 and 0.205 moles of I, are introduced into a 1.00 L vessel at 698 K.

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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