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 following system is initially at equilibrium.
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 following system is initially at equilibrium.
CO(g) + H2O(g) ⇆ CO2(g) + H2(g)
The concentrations of CO, H2O, CO2, and H2 in a 1 L container are 0.60 M, 0.50 M, 1.2 M, and 0.80 M respectively. 0.4 moles of H2 are added to the container. Complete the ICE table to show the changes and equilibrium concentrations using the values from the following list.
![Unit 42-Le Chateliers Principle X
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I
C
E
Answered: ICE tables are used
0.50 0.60 0.80 1.2
[co] | [H,O] [CO,] [H]
+x0.50-x 0.50+x 0.60-x 0.60+x 0.80-x
1.2-x 1.2+x 1.6+x 1.6-x
0.80 + x
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In the given question we have to write the ICE for the following equilibrium reaction.
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