4.1 Chapter 15 Chemical Equilibrium (1 per page)

4.1 Chapter 15 Chemical Equilibrium (1 per page) - Chemical...

Info iconThis preview shows pages 1–10. Sign up to view the full content.

View Full Document Right Arrow Icon
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Chemical Equilibrium: Ch. 15 15-1 Dynamic Equilibrium 15-2 The Equilibrium Constant Expression 15-3 Relationships Involving Equilibrium Constants 15-4 The Magnitude of an Equilibrium Constant 15-5 The Reaction Quotient, Q : Predicting the Direction of a Net Change 15-6 Altering Equilibrium Conditions: Le Châtelier’s Principle 15-7 Equilibrium Calculations: Some Illustrative Examples
Background image of page 2
15-1 Dynamic Equilibrium • Equilibrium – two opposing processes taking place at equal rates. I 2 (H 2 O) I 2 (CCl 4 ) H 2 O(l) H 2 O(g) NaCl(s) NaCl(aq) H 2 O CO(g) + 2 H 2 (g) CH 3 OH(g) Reversible reactions: Both forward and reverse reactions take place I 2 (H 2 O) I 2 (CCl 4 ) Prepared Equilibrium I 2 (H 2 O) I 2 (CCl 4 )
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Dynamic Equilibrium
Background image of page 4
15-2 The Equilibrium Constant Expression • Methanol synthesis is a reversible reaction. CO(g) + 2 H 2 (g) CH 3 OH(g) k 1 CH 3 OH(g) CO(g) + 2 H 2 (g) k -1 N 2 (g) + 3H 2 (g) 2NH 3 (g) As is Ammonia production (Haber-Bosch process) k 1 CO(g) + 2 H 2 (g) CH 3 OH(g) k -1
Background image of page 5

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Three Approaches to Equilibrium ICl H 2 I 2 H 2 (g) + 2 ICl(g) I 2 (g) + 2 HCl(g)
Background image of page 6
The Equilibrium Constant: A kinetic perspective H 2 (g) + 2 ICl(g) I 2 (g) + 2 HCl(g) d t = k [H 2 ][ICl] d[ P ] Mechanism: H 2 (g) + ICl(g) HI(g) + HCl(g) HI(g) + ICl(g) I 2 (g) + HCl(g) k 1 [H 2 ][ICl] = k -1 [HI][HCl] k 2 [HI][ICl] = k -2 [I2][HCl] Step 1 Step 2 At Equilibrium ] [ ] ][ [ ] [ ] ][ [ ] [ 2 2 2 2 2 1 1 1 ICl HCl I k k HCl ICl H k k HI step step = = So, c K k k k k ICl H HCl I = = 2 1 2 1 2 2 2 2 ] ][ [ ] ][ [
Background image of page 7

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Briggs Raucher reaction:Oscillating reactions
Background image of page 8
The Equilibrium Constant and Activities; a Activity – Thermodynamic concept introduced by Lewis. – Dimensionless ratio referred to a chosen reference state. γ B accounts for non-ideal behaviour in solutions and gases. γ B [B] can be considered an effective or active concentration.
Background image of page 9

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 10
This is the end of the preview. Sign up to access the rest of the document.

Page1 / 30

4.1 Chapter 15 Chemical Equilibrium (1 per page) - Chemical...

This preview shows document pages 1 - 10. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online