Question

A, b, c, d all pertain to question 2.

P2. The following equilibrium reaction was established in a closed reaction vessel. H:(g) + 12 (g) 2 HI (g) The equilibrium constant for the reaction is 8.0 x 10-3 (a) (4 points) If the reaction vessel was filled with 4.00 bar of H2. 4.00 bar of lb, and 4.0 bar of HI, which direction will the reaction have shift to reach equilibrium? (Substantiate your answer.) (b) (8 points) Calculate the concentrations for H2, l2, and HI at equilibrium. (Assume that it reaches equilibrium by shifting in the direction you predicted in part (a). 丁 구 G-2x) 3.45S 9-23.qsCHBres +SIA 9 3 H2 디 (c) (2 points) If the reaction above is at equilibrium, and then the volume of the container is reduced which way will the reaction have to shift to re-establish equilibrium? Why? (d) (2 points) If the reaction above is at equilibrium, and then iodine gas starts to solidify on the sides of the container [as in this physical process: 12(g) → 12(s), which way will the reaction have to shift to re-establish equilibrium? Why?

Answer 1

d) If I2 gas is solidified, the concentration on reactant side decreases and hence the reaction shifts towards left side to reach the equilibrium according to Le Chatilier's principle

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