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## PowerPoint Slideshow about ' Chapter 14' - etenia

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I. Equilibrium

- So far we have mostly considered just forward reactions
aA + bB cC + dD

- But all reactions can move in either direction

II. Equilibrium Constant

- Omit concentrations of pure solids and liquids because those concentrations will not change

- Look at elementary steps:

A. What does K mean?

- Large value of K means product favored

2. Small value of K means reactant favored

Example

Given the K of this reaction to be 170, when the conditions are changed what is the Q?

Given the new Q, what is the direction of the reaction to re-establish equilibrium?

IV. Calculations with K

- We need the equilibrium concentrations to determine K, be we usually know initial concentrations, we can therefore get there from the balanced chemical equations!!!

- Butane interconverts to isobutane at 25oC with a K = 2.5. If 0.017 moel of butane is in 50 mL, what is the concentration of both species at equilibrium?

Example

PCl5 (g) PCl3 (g) + Cl2 (g)

K is 1.2 at 25oC. If you place 0.300 M PCl5 (g) in a flask what are the equilibrium concentrations of PCl3 (g), PCl3 (g) and Cl2 (g)?

Example

H2 (g) + Br2(g) 2HBr (g)

- K is 2.18 × 106 at 730oC. If you place 0.267 M HBr (g) in a flask and allow it to come to equilibrium, what are the equilibrium concentrations of H2 (g), Br2 (g) and HBr (g)?

Rules for Manipulating

When the stoichiometric coefficients in a balanced reaction are changed by a factor of n:

- When a chemical reaction is reversed in
- direction:

- When several balanced reactions (each with its own equilibrium constant) are added to obtain a net balanced equation:

Ex

Calculation Knet for the following reaction:

Fe (s) + H2O (g) FeO (s) + H2 (g)

Given the following information:

H2O (g) + CO (g) H2 (g) + CO2 (g) K1 = 1.6

FeO (s) + CO (g) Fe (g) + CO2 (g) K2 = 0.67

VI. LeChatelier’s Principle

- Any change in any of the factors that determine the equilibrium conditions of a system will cause the system to change in such a manner to counteract the effect of the change
- Systems always want to be at equilibrium and will work to get back there.

Example

2SO2 (g) + O2 (g) 2SO3(g) ΔHrxn = -197 kJ

Disturbances:

- Add more SO2(g)
- Take away O2 (g)
- Decrease the volume by ½

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