H6 chemisch evenwicht (1)

Page 1

• Title: CHEMIE H6: Chemisch Evenwicht

• Contains numerical data (200 ml, 50, 150, 100-500, 800, 200, 150, 50, 100) related to experimentation or measurements.

Page 2

• Title: Overzicht

• Sections covered:

  • 6.1. Dynamisch Evenwicht in een Gesloten Systeem (p.215-216)

  • 6.2. Evenwichtsreacties (p.216-217)

  • 6.3. Wet van het Chemisch Evenwicht (p.218-221)

  • 6.4. Verschuiving van het Chemisch Evenwicht (p.222-230)

  • 6.5. Aflopende Reacties (p.231)

  • 6.6. Evenwichtsreacties, Aflopende Reacties, Onmogelijke Reacties (p.232)

  • 6.7. Uitgewerkte Vraagstukken (p.233-234)

Page 3

• Title: Water Evaporation Experiment

• Observation or relevant notes could be mentioned regarding evaporation processes.

Page 4

• Title: Verdamping Water: Open Systeem versus Gesloten Systeem

• Dynamisch Evenwicht in een Gesloten Systeem:

  • Equilibrium between liquid water and water vapor.

  • Statistically no change; evaporation and condensation continue, showing a seemingly stable state = dynamic equilibrium (liquid ⇄ vapor).

Page 5

• Title: Chemische Reacties: Evenwichtsreacties vs Aflopende Reacties

• Reagentia:

  • Reaction: A + B ⇄ C + D

  • Notation indicates the bidirectional conversion of reactants and products.

  • Emphasis on the nature of equilibrium reactions vs. irreversible reactions.

Page 6

• Title: Rate of Reactions

• Dynamics of equilibrium:

  • Rate of forward reaction = Rate of reverse reaction

  • Dynamic Equilibrium concept and its importance in chemical reaction analysis.

Page 7

• Title: Aflopende Reactie vs Evenwichtsreactie

• Aflopende Reactie: All reactants convert completely into products.

• Evenwichtsreactie: Reactants do not completely convert; some remain.

Page 8

• Title: Evenwichtsreacties

• Key Concept: Chemisch Evenwicht

  • A closed system where participating substances aim for equilibrium.

  • Homogeen Evenwicht: Like states of matter (e.g., gases).

  • Heterogeen Evenwicht: Different states of matter (e.g., solid and gas).

Page 9

• Title: Dynamics of Evenwichtsreacties

• Reaction balance:

  • Within a time unit, equal numbers of molecules of A + B convert to C + D and vice versa.

  • Status of dynamic equilibrium where reaction rates equalize.

Page 10

• Title: Voorbeeld Evenwichtsreactie

• Example:

  • Reactants: Fe³⁺ + SCN⁻

  • Products: Fe(SCN)²⁺ (red complex)

  • Visualization of balance between color states of the reaction.

Page 11

• Title: Wet van het Chemisch Evenwicht

• Determining the point when a particular reaction reaches a dynamic equilibrium state.

• General equilibrium reaction given.

Page 12

• Title: Evenwichtsconstante K

• Formula:

  • [P]e^p [Q]e^q / [A]e^a [B]e^b = Kc

  • Indicates the equilibrium condition in terms of concentrations.

Page 13

• Title: Voorbeeldoefening

• In a 1L reaction chamber, initiation scenario for 2SO3(g)↔2SO2(g)+O2(g).

• Calculation of equilibrium constant with given moles.

Page 14

• Title: Oefeningen Vragen

• Specific questions assigned (6.7, p.243)—focus on group collaboration for solutions.

Page 15

• Title: Equilibrium Concepts

• Summary of dynamic equilibriums and reactions.

Page 16

• Title: Herhaling Dynamisch Evenwicht

• Short introduction to dynamic equilibrium.

Page 17

• Title: Verschuiving van het Chemisch Evenwicht

• Clarification of conditions to shift reaction equilibrium.

• Example: Haber-Bosch process favoring ammonia production.

Page 18

• Title: Demoproef

• Experimental setup related to shifting equilibrium of the Fe(SCN) system under various conditions.

Page 19

• Title: Invloed van Concentratieverandering

• Adding/removing reactants causes shifts in equilibrium to offset the change.

• Example with Br2 + H2O.

Page 20

• Title: Verdunning en Druk

• Effects of dilution and pressure changes on equilibrium state; shift towards maximizing particle count.

Page 21

• Title: Invloed Concentratie en Druk

• Short review of principles affecting equilibrium in gas systems.

Page 22

• Title: Invloed Temperatuur en Katalysator

• Overview of temperature and catalyst effects on reaction equilibrium.

Page 23

• Title: Invloed van Temperatuur op het Evenwicht

• Explanation on endothermic and exothermic reactions in terms of temperature changes.

Page 24

• Title: Invloed van een Katalysator

• Katalysators affect reaction rates without shifting equilibrium position.

Page 25

• Title: Wet van Le Chatelier

• Principle detailing equilibrium responses to disturbances; system adjusts to counteract changes.

Page 26

• Title: Oefeningen Vragen

• Assignments for questions on equilibrium; collaboration encouraged.

Page 27

• Title: Toepassing Haber Bosh Process

• Chemical equations related to the Haber process illustrated; focus on ammonia synthesis.