# ICE Tables.

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ICE Tables

Reaction Quotient, Q Q is obtained by applying the law of mass action to INITIAL CONCENTRATIONS! Q is useful in determining which direction a reaction must shift to establish equilibrium. K vs. Q. K is calculated from equilibrium concentrations or pressures. Q is calculated from initial concentrations or pressures.

Reaction Quotient, Q K = Q; The system is at equilibrium. No shift will occur. K < Q; The system shifts to the left. Consuming products and forming reactants, until equilibrium is achieved. K > Q; The system shifts to the right. Consuming reactants and forming products, to attain equilibrium. Write K then Q, the greater/less than sign points the way the reaction shifts!

Change Shift Right 2 H2O ⇌ H3O+ + OH- Shift -2y +y +y Shift Left

K vs Q Problem For the synthesis of ammonia at 500o C, the equilibrium constant is 6.0 x Predict the direction in which the system will shift to reach equilibrium in each of the following cases:  N2(g) + 3 H2(g) ⇌ 2 NH3(g) Conc. (M) [NH3]o [N2]o [H2]o Trial x x x10-3 Trial x x x10-1 Trial x x x10-3

ICE tables To do equilibrium problems set up an ICE table.
Write the balanced equation. Underneath it label three rows. Initial Concentrations (pressure) Change Equilibrium concentration (pressure)

Gas Problem At a certain temperature a 1.00 L flask initially contained mol PCl3, 8.70 x 10-3 mol PCl5, and no Cl2. After the system had reached equilibrium, 2.00 x 10-3 mol Cl2(g) was found in the flask. Gaseous PCl5 decomposes according to the following reaction PCl5(g) ⇌ PCl3(g) + Cl2(g) Calculate the equilibrium concentrations of all species and the value of K.

Answer PCl5(g) PCl3(g) + Cl2(g) 8.7 x10-3 M .298 M 0 -x +x +x I
It must have shifted to the right because chlorine increased. x must = 2.0x10-3 I C E .0067 M .300 M

K K = .3 (.002) / .0067 = .0896

Concentration Problem
Carbon monoxide reacts with steam to produce carbon dioxide and hydrogen. At 700 K the equilibrium constant is Calculate the equilibrium concentrations of all species if mol of each component is mixed in a L flask.

Concentration Problem
Assume that the reaction for the formation of gaseous hydrogen fluoride from hydrogen and fluorine has an equilibrium constant of 1.15 x 102 at a certain temperature. In a particular experiment, mol of each component was added to a L flask. Calculate the equilibrium concentrations of all species.

Quadratic Equation To solve some problems you need to use the quadratic equation or solver function on a calculator For a x2 + bx + c = 0 x = -b   b2 – 4ac 2a

Graphing calculators (required for this course) come with a solver function to solve equations. You can also have a quadratic equation program. All of this is legal for the AP or any of my tests. *except on multiple choice, but I have not seen that.

Simplified Assumptions
If you are using a solver function this is unnecessary. You do have to understand the concept for a possible multiple choice For some reactions the change will be very small compared to the initial amount. You always have to check!

Example Gaseous NOCl decomposes to from the gases NO and Cl2. At 35o C, the K = 1.6 x The initial conc. Of NOCl is .5 M. What are the equilibrium concentrations? 2NOCl(g) ⇌ 2NO(g) + Cl2(g) The small K value means this will favor the reactant side so there wouldn’t be a large shift to the right.

Problem 2NOCl(g) ⇌ 2NO(g) + Cl2(g) I .50 0 0 C -2x +2x + x
E x x x 1.6 x10 -5 = (2x)2 x / (.5-2x)2 The algebra looks a little sticky on this problem If the shift is really small then .50 -2x  .5

Solve now 1.6 x10 -5 = (2x)2 x / (.5)2 x = .01
Of course this is ONLY ACCEPTABLE IF x  .5 .50 – 2 (.01) = .48 If the change is less than 5% it is considered small enough to ignore .48/.5 = 96% or a 4% change.

Solver Function This equation 1.6 x10 -5 = (2x)2 x / (.5-2x)2
is not difficult to solve using a solver function. You have to have a decent guess, you may have to change your guess. You canNOT have a negative value for your shift.

Simplified Assumptions
In a study of halogen bond strengths, 0.50 mol I2 was heated in a 2.5 L vessel, and the following reaction occurred: I2(g) ⇌ 2I(g). Calculate [I2]eq and [I]eq at 600 K; Kc = 2.94 x Calculate [I2]eq and [I]eq at 2000 K; Kc =