Answer to Question #74520 in General Chemistry for seper

Question

Consider the following equilibrium system that has an equilibrium constant, Keq, of 11.2:

H2(g) + B2(g) 2HBr


The initial concentrations are as follows:

[H2(g)] = 0.200M, [B2(g)] = 0.300M & [HBr(g)] = 1.20M

Predict which direction the system will shift to achieve equilibrium.

b) Calculate the concentration of each species at equilibrium.

c) If 0.100 moles of H2 gas was injected into the system, calculate the concentrations of each gas when the second equilibrium has been reached.

d) After the second equilibrium was reached a student added an unknown amount of HBr gas. He found that the concentration of Br2 gas increased by 0.025 M. How much HBr gas did the student add to the system?

e) Draw the concentration vs time graph to show how this system achieved the first, the second equilibrium, and the third equilibrium.

Answer 1

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