'Reaction quotient' diaporamas de présentation

Chemical Equilibrium. Chapter 14 14.1-14.5. Equilibrium. Equilibrium is a state in which there are no observable changes as time goes by. Chemical equilibrium is achieved when: 1.) the rates of the forward and reverse reactions are equal and

Reaction Rates & Equilibrium. Rates of Reaction (rxn.) Reversible Reactions and Equilibrium Determining Whether a Reaction Will Occur Calculating Entropy and Free Energy The Progress of Chemical Reactions. Chemical Equilibria. Reactions going to completion ( ↓ )

Chapter 14 Notes. Fundamentals of Electrochemistry. Redox Reactions. Reactions involving the transfer of electrons from one species to another. LEO says GER Oxidation – Loss of electrons Reduction – Gain of electrons. Definitions.

Intro Lab Schedule for winter 2011 . Monday sections : Sections 51 and 52 - Monday, January 7 @ 2:30 p.m. Sections 55 and 56 - Monday, January 7 @ 3:15 p.m. Tuesday sections Sections 53 and 54 - Tuesday, January 8 @ 2:30 p.m. Sections 57 and 58 - Tuesday, January 8 @ 3:15 p.m.

Equilibrium. Unit 10. Reaction Dynamics. If the products of a reaction are removed from the system as they are made, then a chemical reaction will proceed until the limiting reactants are used up.

JCHS Honors Chemistry Spring Final S.G (Part 2). CH Williams. CHEMICAL EQUILIBRIUM. Cato Maximilian Guldberg and his brother-in-law Peter Waage developed the Law of Mass Action. Chemical Equilibrium. Reversible Reactions: . A chemical reaction in which the products

Chemical Equilibrium. The reversibility of reactions. Equilibrium. Many chemical reactions do not go to completion. Initially, when reactants are present, the forward reaction predominates. As the concentration of reactants increases, the reverse reaction begins to become significant.

Chemical Equilibrium. Chapter 6 E-mail: benzene4president@gmail.com Web-site: http://clas.sa.ucsb.edu/staff/terri/. Chemical Equilibrium – Ch. 6. 1. Consider the following reaction: N 2 (g) + 3 Cl 2 (g) 2 NCl 3 (g) a. Write the equilibrium expression (K c and K p )

More Ksp. Comparing Solubilities. The relative solubilities can be deduced by comparing values of K sp . BUT, BE CAREFUL! These comparisons can only be made for salts having the same ION:ION ratio. Comparing Solubilities. Which salt is more soluble? Ag 2 S Ksp = 1.0 X 10 -49

Chemistry 100 Chapter 19 . Spontaneity of Chemical and Physical Processes: Thermodynamics. What Is Thermodynamics?. Study of the energy changes that accompany chemical and physical processes. Based on a set of laws.

Kinetics II. Lecture 15 . Rates and Concentrations. Knowing the rate constant (usually empirically determined), we can compute rate. Integrating rate of first order reaction gives: Graph shows how CO 2 concentration changes in the reaction CO 2 + H 2 O = H 2 CO 3.

Chemistry 142. Review. Chapter 13: Chemical Kinetics . Rate Relativ e Rate of Reaction Law of Mass Action and Instantaneous Rate of Reaction Rate Law Reaction order Effect of nature of reactants, temperature, molecular orientation, concentration, catalyst

Applications of Equilibrium Constants. Example. For the reaction below 2A + 3B  2C A 1.5L container is initially charged with 2.3 mole of A and 3.0 mole of B. At equilibrium, .75 mole of A is present. Calculate the value of the equilibrium constant. Example.

Intersection 15: The End. 12/12/06. The Final Exam Questions. Electron configurations, atomic structure, periodic trends, atomic orbitals. Quantitative calculations. Lewis & VSEPR Structures and polarity. Thermochemistry Thermochemistry Thermochemistry Acid/Base chemistry

Lecture 7 Chemical Equilibrium. Define equilibrium constant – K Define the free energies: D G f  , D G r  and D G r Calculate K from D G r  Define Q – How is it different from K Goal – Learn how to do equilibrium calculations! Sounds hard but the tools to use are

Chapter 15 Principles of Chemical Equilibrium. Contents in Chapter 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

“Thermodynamics II”. Entropy, Free Energy, and Equilibrium. Chapter 18. First Law of Thermodynamics. Energy can be converted from one form to another but energy cannot be created or destroyed. D E = q + w. D E the change in internal energy of a system.

Standard Reference Electrode Standard Hydrogen Electrode (SHE). SHE: • Assigned 0.000 V • Can be anode or cathode • Pt does not take part in reaction • Difficult to operate. Standard Conditions: 1 atm for gases, 1.0M for solutions, 25 o C for all (298 K).

Reaction Rates and Equilibrium. M.Elizabeth 2011. Collision Theory Used to Explain Reaction Rates. Atoms, ions, and molecules can form a chemical bond when they collide , provided the particles have enough kinetic energy .

Chapter 13. Chemical Equilibrium. Chemical Equilibrium. Chemical equilibrium occurs in chemical reactions that are reversible. In a reaction such as: CH 4 (g) + H 2 O(g)  CO(g) + 3H 2 (g) The reaction can proceed in both directions CO(g) + 3H 2 (g)  CH 4 (g) + H 2 O(g).