The following reaction has an equilibrium constant, Kc, of 2.10 x 102 at a particular temperature: N2 (g) + 3 H2 (g) → 2 NH3 (g) + You have a container in which the concentration of N2 is 0.77 M, the the concentration of H2 is 0.84 M, and the concentration of NH3 is 0.85 M. (a) Calculate the value of the reaction quotient Q. (b) Is the system at equilibrium? If not, predict which way (right or left) the reaction will proceed to reach equilibrium.
The following reaction has an equilibrium constant, Kc, of 2.10 x 102 at a particular temperature: N2 (g) + 3 H2 (g) → 2 NH3 (g) + You have a container in which the concentration of N2 is 0.77 M, the the concentration of H2 is 0.84 M, and the concentration of NH3 is 0.85 M. (a) Calculate the value of the reaction quotient Q. (b) Is the system at equilibrium? If not, predict which way (right or left) the reaction will proceed to reach equilibrium.
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 13Q: Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this...
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The following reaction has an equilibrium constant, Kc, of 2.10 x 102
at a particular temperature:
N2 (g) + 3 H2 (g) → 2 NH3 (g) +
You have a container in which the concentration of N2 is 0.77 M, the the concentration of H2 is 0.84 M, and
the concentration of NH3 is 0.85 M.
(a) Calculate the value of the reaction quotient Q.
(b) Is the system at equilibrium? If not, predict which way (right or left) the reaction will proceed to
reach equilibrium.
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