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H 2(g) + I 2(g) 2HI (g) Write the K expression [H 2 ] = M [I 2 ] = M [HI] = 1.29 M
H 2(g) + I 2(g) 2HI (g) What is the equilibrium conc of [HI] if: [H 2 ] = 0.81 M [I 2 ] = M
Solve for K if: It is the reverse rxn The eqn is 1/3 of the original The eqn is reversed and is 4 times the original.
Equilibria with pressures? So far, we’ve only used concentration gases can be described in terms of pressures
PV = nRT P =(n/V]RT = CRT C= molar conc of gas K p is the equilibrium in terms of partial pressures of the gases
N 2(g) + 3H 2(g) 2NH 3(g) Write the K p expression How do K and K p relate? Let’s try it for this rxn… K= K p (RT) 2
H 2(g) + F 2(g) 2HF (g) Try it for this rxn… K = K p b/c sum of coefficients on either side is equal
General relationship K p = K(RT) n n= the sum of the coefficients of the gaseous products minus the sum of the coefficients of the gaseous reactants
CH 3 OH (g) CO (g) + 2H 2(g) At 25 o C P CH3OH = 6.10 x atm P CO = atm P H2 = 1.34 atm What is K?
So far... Our systems have only involved gases! Homogeneous equilibria- where phases are all the same
Heterogeneous equilibria Equilibria involving more than one phase Take for instance… CaCO 3(s) CaO (s) + CO 2(g) Write the K
However... Experiments show that the position of heterogeneous equilibrium does not depend on the amounts of pure solids or liquids present!!
Why?? Concentrations of pure solids and liquids can NOT change!! So… LEAVE THEM OUT of K!! Let’s try…
Homework P 640 (WOW!) 22, 25, 28, 29, 31
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Chemical Equilibrium Reactions Go Both Ways Equilibrium Plural is equilibria (for you Latin fans) Reactions are reversible –they go forward and backward.
H 2 O + CO H 2 + CO 2 As a reaction proceeds, the concentration of reactants declines, and the concentration of products increases.
Equilibrium Chemical Equilibrium. General Info on Equilibrium Concerned with how far a reaction goes. Why does it have a low or high % yield? Why do some.
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CHEMICAL EQUILIBRIUM. Chemical Equilibrium Reversible Reactions: A chemical reaction in which the products can react to re-form the reactants Chemical.
Rates & Extents of Reactions. Rates & Extents of Rates & Extents of Reactions Quiz A Quiz A What prevents reaction from What prevents reaction from going?
Equilibrium Chapter 12. Equilibrium Chemical equilibrium is a dynamic condition in which concentrations do not change and the rates of the forward and.
AP Notes Chapter 16 Equilibrium Dynamic chemical system in which two reactions, equal and opposite, occur simultaneously.
Topic 22 Topic 22 Topic 22: Chemical Equilibrium Basic Concepts Additional Concepts Table of Contents Topic 22 Topic 22.
Equilibrium. Equilibrium Some reactions (theoretically all) are reversible reactions, in which the products take part in a separate reaction to reform.
Chemical Equilibrium Unit 2. One way reactions b Reactants react forming products. b The reaction continues until one of the reactants is finished. b.
Chemical Equilibrium A B + A B + C D + A B + C D + Reaction begins. No products yet formed. High rate of collisions between A & B. Rate of forward reaction.
Reaction Rates and Equilibrium M.Elizabeth Collision Theory Used to Explain Reaction Rates Atoms, ions, and molecules can form a chemical bond when.
o If you recall, we mentioned that there are rxns that bounce back and forth from forming products to reforming reactants A.K.A. reversible rxns A.K.A.
Drill – 5/28 1. Write the equilibrium expression for sulfuric acid.
For an ideal gas, molarity is directly proportional to pressure M = P RT therefore K c is directly related to K c by the equation: K p = K c (RT) n.
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Unit 6: Equilibrium applications Ksp Ksp: review (grade 11) 1) What is the molar mass of H 2 O? 2) How many moles are in 18 g of NaCl? 3) How many g.
1 Le Châtelier. 2 Standard Know how to use Le Châtelier’s principle to predict the effect of changes in concentration, pressure, and temperature. Know.
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