# Equilibrium Lecture #1. Schweitzer

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1 Equilibrium Lecture #1 Schweitzer

2 What is equilibrium? Remember Equilibrium process between to competing reactions. At equilibrium the forward process is equal to the reverse process. *** It appears that nothing is happening***

3 Practice Problem (Ebbing14.10) A state of dynamic equilibrium exists at constant temperature in 1. a stoppered flask half full of water 2. an open pan of boiling water. 3. a stoppered flask of a solution of sodium carbonate solution a. 1 only d. 1 and 2 only b. 2 only e. 1 and 3 only c. 3 only

4 Practice Problem (Ebbing14.10) A state of dynamic equilibrium exists at constant temperature in 1. a stoppered flask half full of water 2. an open pan of boiling water. 3. a stoppered flask of a solution of sodium carbonate solution a. 1 only d. 1 and 2 only b. 2 only e. 1 and 3 only c. 3 only

5 Writing equilibrium Expressions 2A(s) + B(aq) <=> 2C(g) + D(aq) Kc Notice: There are now substances on both sides of the reaction. This is a K for a general reaction c stands for general concentrations. Kc = [C] 2 [D]/[B] Note: The solid does not show up in Equilibrium Expression.

6 Kc What is the difference between Kc and Kp Measures all units in Moles/Liter Can not include pure solids and liquids Kp Measures all units in Atmospheres Only includes gases

7 Practice writing equilibrium expressions 2A(s) + B(aq) <=> 2C(g) + D(aq) Kp This is a K for a general reaction p stands for Pressure (atmospheres). Kp = [C] 2 /1 Note: Only include gases

8 Write an equilibrium expression 2A(g) + B(s) 2C(l) + D(aq) Kc = [D]/[A] 2 Kp = 1/[A] 2 Remember: all units are in ATM and only gases are used

9 Problems involving Equilibrium What information can a problem give you? They can give you the equilibrium constant. They can give you initial conditions They can give you equilibrium conditions Note: Equilibrium conditions can be put directly into the equilibrium expression. THE FOLLOWING PROBLEMS ARE GOING TO BE DIFFERENT COMBINATIONS OF THIS INFORMATION. THERE ARE NOT THAT MANY DIFFERENT TYPES OF PROBLEMS KEEP TRACK...

10 Solving for Concentration given: K and starting materials CO(g) + H 2 O (g) H 2 (g) + CH 4 (g) Suppose you start with1 mol of each CO and water in a 50.0L vessel. How many moles of each substance are in the equilibrium mixture at 1000C? Kc = 0.58 What are they giving you here in this problem?

11 Answer CO(g) + H 2 O (g) H 2 (g) + CH 4 (g) 1/50 I C -x -x x x E (.02-x) (.02-x) x x Kc = [H 2 ][CH 4 ]/[H 2 O][CO].58 = x 2 / (.02-x) (.02-x) Solve for X Notice the short cut can NOT be used in this problem

12 Look for alternate methods.58 = x 2 / (.02-x) (.02-x) Solve for X.58 = x 2 / (.02-x) 2 Square root both sides = x/ x Solve for x (x must be positive) = Substitute into the equilibrium expression CO(g) + H 2 O (g) H 2 (g) + CH 4 (g)

13 Practice problem Ebbing597 Carbon monoxide and hydrogen react according to the following equation CO(g) + 3H 2 (g) CH 4 (g) + H 2 O(g) When 1 mol CO and 3 mol of H 2 are placed in a 10 L vessel at 927C and allowed to come to equilibrium, the mixture is found to contain mol of H 2 O. What is the concentration of each substance at equilibrium and what is Kc for the reaction.

14 Answer CO(g) + 3H 2 (g) CH 4 (g) + H 2 O(g) I..1M.3M 0 0 C -x -3x x x E.0613?.184?.0387?.0387 Note: This is simply a stoichiometry problem = * 3 =.1161

15 More Practice!!! (Ebbing603) Hydrogen Iodide decomposes at a moderate temperature according to the following reaction 2HI(g) H 2 (g) + I 2 (g) When 4.00mol of HI was placed in a 5.00L vessel at 458C, the equilibrium mixture was found to contain mol of I 2. What is the value of Kc for this reaction at the specified temperature?

16 Answer 2HI(g) H 2 (g) + I 2 (g) I C -2x +x +x.0844 E Plug these concentrations into Kc expression Kc =.0201

17 What if they give you equilibrium concentrations? An equilibrium mixture of gases contains.30 mol CO, 0.10 mol of H 2, and 0.20 mol H 2 O, plus an unknown amount of CH 4. The total volume of the system is 1 Liter. Kc for this reaction = 3.92 CO(g) + 3H 2 (g) H 2 O(g) + CH 4 (g)

18 Answer I C CO(g) + 3H 2 (g) H 2 O(g) + CH 4 (g) E ? Note: These are all equilibrium conditions. These can be plugged directly in the Kc expression = [CH 4 ][.02]/[.30][.10] 3 CH 4 = 0.059M

19 Calculating percent change Very often the percent change will be used to tell the extent of a reaction (amount it moves to product) Or they will want you to calculate % Change % change = Change/original x 100

20 Using percent change Reaction A(g) = 2B(g) + C(g) is ran at 100C and the initial concentration of A was.1m. Kc(A) = 1.0 E-8) What is the percent change of A in this reaction at equilibrium

21 Answer % change = Change/original x 100 A(g) = 2B(g) + C(g) I C -x +2x +x E.1-x 2x x 1.0E-8 = [2x] 2 [x]/.1 1.0E-8 = 4x 3 /.1

22 Predicting the direction of a reaction using reaction quotient We used the reaction quotient when we predicted whether a reaction would precipitate or not. If Q > K Then the mixture has too much product and will therefore shift toward reactant. If Q < K Then the mixture has too much reactant and will therefore shift toward product.

23 Practice (Ebbing610) A 50.0L reaction vessel contains 1.0 mol N 2, 3.00 mol H 2, and.500 mol of NH 3. Will more ammonia, NH 3 be formed or will it dissociate when the mixture goes to equilibrium? The equilibrium constant(k) = 0.500

24 Answer Q = [NH 3 ] 2 /[N 2 ][H 2 ] 3 Q = (0.0100) 2 /(0.0200)(0.0600) 3 Q = 23.1 And K = So Q > K So we have to much product. Reaction will shift back toward reactant

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