CHEM 121 Chapter 6.

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Presentation transcript:

CHEM 121 Chapter 6

Energy Ability to do work Potential Energy: Kinetic Energy: Heat: Law of conservation of energy:

Energy Units Joule Kilojoule calorie Calorie

Nutritional Calories Cal/g A label on a bag of chips says that it contains 16 g fat, 34 g carbs, 4 g protein, and has a total of 300 Calories. Are the nutrition facts accurate?

Spontaneity Spontaneous process: Nonspontaneous process: Exergonic: Endergonic:

Collision Theory Reactions occur when molecules: Energy Diagram Activation Energy:

Enzyme Reactions

Energy Diagrams

Bond Energies E needed to break bonds E released to make bonds Bond Dissociation Energy

Energy Change in Reactions H + Cl ΔH = -103 kcal/mol 2 NH3 (g) ΔH = 22 kcal/mol Products: Reactant:

Reaction Rate Speed of a reaction Measured by the time needed:

What affects reaction rates?

Reversible Reactions Many reactions can go forward AND backwards Chemical Equilibrium

Chemical Equilibrium

Equilibrium Constants coefficients reactants products

Practice Balance and write the equilibrium expression for each of the following: The reversible reaction of phosphorous trichloride combining with chlorine to form phosphorous pentachloride. (All are gases.)

Equilibrium Homogeneous equilibrium: Heterogeneous equilibrium:

Calculating Equilibrium Constants N2O4 (g) NO2 (g) 2 Must be determined experimentally At 100 °C, once this reaction reaches equilibrium, the concentration of N2O4 is 0.45 M and NO2 is 0.31 M. What is the value of Kc?

Equilibrium Constants Large Kc value: Greater concentration of reactants or products?

Equilibrium Constants Small Kc value: Greater concentration of reactants or products?

Practice Will each of the following favor reactants or products? Reaction with Kc = 2.9 x 10-12 Reaction with Kc = 0.001 x 105

Calculating Concentrations at Equilibrium Carbon monoxide and hydrogen gas react reversibly to form CH4 (g) and water vapor. What is the concentration of CH4 at equilibrium? At equilibrium at 1000 °C, the concentrations of hydrogen, carbon monoxide, and water are 0.30 M, 0.51 M, and 2.0 M, respectively. (Kc at 1000 °C = 260)

Le Châtelier’s Principle At equilibrium, concentrations of substances do not change. If a stress is put on the reaction at equilibrium, the equilibrium will _______________________ What changes count as stress?

Effect of Concentration Changes NO2 (g) NO (g) + O2 (g) What is the effect on the equilibrium? Add NO2? Add O2? Remove NO2? Remove NO?

Effect of Pressure Changes If P increases, equilibrium shifts to side with ____________________________ If P decreases, equilibrium shifts to side with ____________________________ NO2 (g) NO (g) + O2 (g)

Effect of Temperature Changes If T increases, equilibrium shifts to _____________ If T decreases, equilibrium shifts to _____________ Endothermic: A (g) B (g) + C (g) Increase the temperature?

Practice Consider the exothermic reaction between nitrogen gas and hydrogen gas, creating ammonia gas (NH3). Write a balanced equation for this reaction. Which direction will the equilibrium shift if: T is increased? Ammonia is removed? A catalyst is used? Hydrogen is added?