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ICE tables are used for calculating changes in concentration in an equilibrium system. I represents the initial concentration, C the change in concentration between the initial value and the equilibrium value, and E the final concentration at equilibrium. The equilibrium constant, K, for the following hypothetical system is 12.0 at 373 K. A(g) + 3 B(g) = C(g) + 2 D(g) The initial concentrations of A, B, C, and D are 0.80 M, 0.40 M, 2.0 M, and 0.60 M respectively. Calculate the value of Q and compare with K to determine if the system moves to the left or the right to achieve equilibrium. Then complete the ICE table to show the changes and equilibrium concentrations using the values from the following list.

ICE tables are used for calculating changes in concentration in an equilibrium system. I represents the initial concentration, C the change in concentration between the initial value and the equilibrium value, and E the final concentration at equilibrium. The equilibrium constant, K, for the following hypothetical system is 12.0 at 373 K. A(g) + 3 B(g) = C(g) + 2 D(g) The initial concentrations of A, B, C, and D are 0.80 M, 0.40 M, 2.0 M, and 0.60 M respectively. Calculate the value of Q and compare with K to determine if the system moves to the left or the right to achieve equilibrium. Then complete the ICE table to show the changes and equilibrium concentrations using the values from the following list.

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.36PAE: The experiment in Exercise 12.33 was redesigned so that the reaction started with 0.15 mol each of...
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So these ICE charts are a killer for me. I seem to be understanding every it these so please show you work a little but not to much. Thank you

ICE tables are used for calculating changes in concentration in an equilibrium system. I represents the initial concentration, C the change in concentration between the initial value and the equilibrium value, and E the final concentration at equilibrium. The equilibrium constant, K, for the following hypothetical system is 12.0 at 373 K. A(g) + 3 B(g) = C(g) + 2 D(g) The initial concentrations of A, B, C, and D are 0.80 M, 0.40 M, 2.0 M, and 0.60 M respectively. Calculate the value of Q and compare with K to determine if the system moves to the left or the right to achieve equilibrium. Then complete the ICE table to show the changes and equilibrium concentrations using the values from the following list.
Transcribed Image Text:ICE tables are used for calculating changes in concentration in an equilibrium system. I represents the initial concentration, C the change in concentration between the initial value and the equilibrium value, and E the final concentration at equilibrium. The equilibrium constant, K, for the following hypothetical system is 12.0 at 373 K. A(g) + 3 B(g) = C(g) + 2 D(g) The initial concentrations of A, B, C, and D are 0.80 M, 0.40 M, 2.0 M, and 0.60 M respectively. Calculate the value of Q and compare with K to determine if the system moves to the left or the right to achieve equilibrium. Then complete the ICE table to show the changes and equilibrium concentrations using the values from the following list.
-X +X I C E -2x +2x [Α] 0.80 -3x +3x 0.40-x 0.60-2x 0.60 + 2x [B] 0.40 0.80-x [C] 2.0 0.40 - 3x 0.40 + x 0.80 + x 0.40 + 3x 2.0-x 2.0 + X [D] 0.60 0.60-x 0.60 + x
Transcribed Image Text:-X +X I C E -2x +2x [Α] 0.80 -3x +3x 0.40-x 0.60-2x 0.60 + 2x [B] 0.40 0.80-x [C] 2.0 0.40 - 3x 0.40 + x 0.80 + x 0.40 + 3x 2.0-x 2.0 + X [D] 0.60 0.60-x 0.60 + x
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