Chemistry 122 Review Chapter 9. Organic Chemistry - Vocabulary Organic, cracking, hydrocarbon, refining, reforming, saturated, hydrogenation, aromatic,

Slides:



Advertisements
Similar presentations
Le Chatelier’s Principle Chem 12 Chapter 13, Pg
Advertisements

Equilibrium Chemistry 30.
AP CHEMISTRY CHAPTER 6 NOTES THERMOCHEMISTRY
Chapter 8 Stoichiometry.
Ch. 16: Energy and Chemical Change
International Baccalaureate Chemistry International Baccalaureate Chemistry Topic 7 – Chemical Equilibrium.
Equilibrium A state in which opposing processes of a system are occurring at the same rate. 1.Physical (a) Saturated Solution – dissolution and crystallization.
Equilibrium Chemistry. Equilibrium A + B  AB We may think that all reactions change all reactants to products, or the reaction has gone to completion.
Warm up u P 4 + N 2 O  P 4 O 6 + N 2 u Balance the equation. u What is the Limiting/Excess reactant for 12 mol P 4 and 14 mole N 2 O.
Thermochemistry “The Quick and Dirty”.  Energy changes accompany every chemical and physical change.  In chemistry heat energy is the form of energy.
Enthalpy C 6 H 12 O 6 (s) + 6O 2 (g) --> 6CO 2 (g) + 6H 2 O(l) kJ 2C 57 H 110 O O 2 (g) --> 114 CO 2 (g) H 2 O(l) + 75,520 kJ The.
Chapter 11 (Practice Test)
CHAPTER 17 THERMOCHEMISTRY.
Bomb Calorimetry constant volume often used for combustion reactions heat released by reaction is absorbed by calorimeter contents need heat capacity of.
Enthalpy Calculations
Chemistry Review Part 4: Molar Relationships The mole and molar calculations Stoichiometry Solution Concentrations Chemical Equilibrium \ You will need.
Stoichiometry II. Solve stoichiometric problems involving moles, mass, and volume, given a balanced chemical reaction. Include: heat of reaction Additional.
Chapter 17 Thermochemistry 17.3 Heat in Changes of State
Energy Chapter 16.
Jeopardy ChemicalPhysicalFormulasEquations Chemistry Q $100 Q $200 Q $300 Q $400 Q $500 Q $100 Q $200 Q $300 Q $400 Q $500 Final Jeopardy.
Section 11.1 The Flow of Energy - Heat
Thermochemistry.
The study of the heat flow of a chemical reaction or physical change
Chapter 17 Thermochemistry.
Chapter 17 - Thermochemistry Heat and Chemical Change
Unit 13: Thermochemistry Chapter 17 By: Jennie Borders.
Dynamic Equilibrium. Objectives Describe chemical equilibrium in terms of equilibrium expressions Use equilibrium constants Describe how various factors.
Honors Chapter 12 Stoichiometry u Greek for “measuring elements” u The calculations of quantities in chemical reactions based on a balanced equation.
Chapter 8 Thermochemistry. Thermodynamics  Study of the changes in energy and transfers of energy that accompany chemical and physical processes.  address.
Thermochemical equations Thermochemical equations  Thermochemical equation = a balanced chemical equation that includes the physical states.
Chapter 11 - Thermochemistry Heat and Chemical Change
Chapter 17 “Thermochemistry” Pequannock Township High School Chemistry Mrs. Munoz.
Mullis1 First Law of Thermodynamics (Law of Conservation of Energy) The combined amount of matter and energy in the universe is constant. The combined.
Mole, gas volume and reactions, Chemical energy and Enthalpy,
TO LIVE IS THE RAREST THING IN THE WORLD. MOST JUST EXIST. THAT IS ALL.
Chapter 17 “Thermochemistry”. 2 Energy Transformations u “Thermochemistry” - concerned with heat changes that occur during chemical reactions u Energy.
200 I’m gassy Let’s bond Stoichiometry Energizer Bunny I have the.
Chemical Kinetics and Collision Theory Aim KE1 How do chemical reactions actually happen?
Thermochemistry Energy in State Changes. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Heats of Fusion and Solidification.
Chapter 18 – Rates of Reactions and Equilibrium Every biological and non-biological chemical reaction in nature eventually reaches a state called equilibrium.
Unit 13: Thermochemistry Chapter 17 By: Jennie Borders.
Chapter 17 - Thermochemistry -is the study of energy relationships in chemical and physical reactions.
Calorimetry.
1 Chapter 11 Introduction to Organic Chemistry: Alkanes 11.4 Properties of Alkanes Copyright © 2007 by Pearson Education, Inc. Publishing as Benjamin Cummings.
1 CHAPTER 4 Solutions B By Dr. Hisham Ezzat First year.
Keeping your balance. Equilibrium Systems at equilibrium are subject to two opposite processes occurring at the same rate Establishment of equilibrium.
Reversible Reactions and Equilibrium
Stoichiometry u Greek for “measuring elements” u The calculations of quantities in chemical reactions based on a balanced equation. u We can interpret.
Thermochemistry Chapters 16 and 17 Thermodynamics – the study of energy and energy transfer. Thermochemistry – the study of energy involved in chemical.
Thermal Chemistry. V.B.3 a.Explain the law of conservation of energy in chemical reactions b.Describe the concept of heat and explain the difference between.
Energy The ability to do work or produce heat The ability to do work or produce heat Potential- Stored energy Potential- Stored energy Energy stored in.
Chemistry 231 Thermodynamics in Reacting Systems.
Chapter 17 Review “Thermochemistry”. Chapter 17 Review What would likely happen (how would it feel) if you were to touch the flask in which an endothermic.
Chemical Equilibrium. n In systems that are in equilibrium, reverse processes are happening at the same time and at the same rate. n Rate forward = Rate.
Thermochemistry Part 4: Phase Changes & Enthalpies of Formation.
Thermochemistry Some Like It Hot!!!!!. The Flow of Energy ► Thermochemistry – concerned with heat changes that occur during chemical reactions ► Energy.
Thermochemistry Chapter 17. Introduction Thermochemistry is the chemistry associated with heat. Heat (q) is a form of energy that flows. Heat flow is.
Chapter 17: Thermochemistry
Chemical Reactions Chapter 7. Describing Chemical Reactions  What type of change is happening in the picture to the left?  Chemical Reaction  New Products.
Chapter 17: Thermochemistry 17.1 The Flow of Energy – Heat and Work.
Chemistry Unit 8 Thermochemistry Chapter The Flow of Energy Energy Transformations – Goal 1 Chemical Potential Energy Energy stored in chemical.
THERMOCHEMISTRY. Law of conservation of energy Energy can be neither created or destroyed but can be converted from one form to another. Energy in = Energy.
Collision Theory  Collision theory is a theory proposed independently by Max Trautz in 1916 and William Lewis in 1918, that qualitatively explains how.
Heat in Chemical Reactions. Heat: the transfer of energy to a substance causing an increase in that substance’s average kinetic energy Temperature: a.
Chapter 15 Energy and Chemical Change Section 15.1 Energy Section 15.2Heat Section 15.3Thermochemical Equations Section 15.4 Calculating Enthalpy Change.
6/14/20161 Chapter 10- Causes of Change Heat and Chemical change.
Topics 5 and 15. Hess’s Law Calorimetry Enthalpy Enthalpy of Formation Bond Energy.
Welcome to Thermochemistry!. Energy in Chemistry Energy in Chemistry (11:23)  Energy is the ability to do work or produce heat. The sum of the potential.
Unit IV – Chapter 7 Section 7.3
Presentation transcript:

Chemistry 122 Review Chapter 9

Organic Chemistry - Vocabulary Organic, cracking, hydrocarbon, refining, reforming, saturated, hydrogenation, aromatic, phenyl, functional group Organic, cracking, hydrocarbon, refining, reforming, saturated, hydrogenation, aromatic, phenyl, functional group

Organic Chemistry - Structures Alkanes: single bonded carbons. General formula C n H 2n+2 Alkanes: single bonded carbons. General formula C n H 2n+2 If branches: (# of location) - (branch name) (parent chain) If branches: (# of location) - (branch name) (parent chain) Parent chain is always longest chain Parent chain is always longest chain Cycloalkanes: Single C-C bonds that form ring. Formula of C n H 2n Cycloalkanes: Single C-C bonds that form ring. Formula of C n H 2n

Organic Chemistry - Structures Alkenes - hydrocarbons with one or more double carbon-carbon bonds (C=C). General form: C n H 2n Alkenes - hydrocarbons with one or more double carbon-carbon bonds (C=C). General form: C n H 2n Alkynes - hydrocarbons with one or more triple carbon-carbon bonds (C=C). General form: C n H 2n-2 Alkynes - hydrocarbons with one or more triple carbon-carbon bonds (C=C). General form: C n H 2n-2 Benzene - Formula C 6 H 6 Benzene - Formula C 6 H 6

Organic Chemistry - Structures Organic Halides - organic compounds that contain one or more halogen atoms Organic Halides - organic compounds that contain one or more halogen atoms Aldehydes and Ketones - Both contain the carbonyl functional group (C=O) Aldehydes and Ketones - Both contain the carbonyl functional group (C=O) In aldehydes the carbonyl group is on the end of the chain, in ketones it is not at the end of the chain. In aldehydes the carbonyl group is on the end of the chain, in ketones it is not at the end of the chain.

Organic Chemistry - Structures Carboxylic acids - Contain both carbonyl (C=O) and hydroxyl (OH) groups Carboxylic acids - Contain both carbonyl (C=O) and hydroxyl (OH) groups O O || || Esters - Contain -C-O-R Esters - Contain -C-O-R Amide - has a carbonyl group bonded to a nitrogen Amide - has a carbonyl group bonded to a nitrogen Amine - has a nitrogen bonded to one or more carbons Amine - has a nitrogen bonded to one or more carbons

Examples to Try…. 3-ethyl-2,4-dimethylhexane 3-ethyl-2,4-dimethylhexane cyclopentane cyclopentane CH 2 =CH-CH 2 -CH 3 CH 2 =CH-CH 2 -CH 3 1,2-dimethylbenzene 1,2-dimethylbenzene CH 3 -CH-CH 2 -CH 2 -CH 3 CH 3 -CH-CH 2 -CH 2 -CH 3

Examples to Try…. C 2 H 5 Br C 2 H 5 Br CH 3 -CH 2 -OH CH 3 -CH 2 -OH 1,2-ethanediol 1,2-ethanediol

Chemistry 122 Review Chapter 10

Vocabulary Chemical system, energy, exothermic, endothermic, specific heat capacity, volumetric heat capacity, phase change, enthalpy, fusion, vaporizing, condensation, molar enthalpy, heating curve Chemical system, energy, exothermic, endothermic, specific heat capacity, volumetric heat capacity, phase change, enthalpy, fusion, vaporizing, condensation, molar enthalpy, heating curve

Main Formulas The heat change in a chemical system may be quantified using either of the following equations: The heat change in a chemical system may be quantified using either of the following equations: q = m c s  t or q = v c v  t q = m c s  t or q = v c v  tWhere: q = quantity of heat flowing to or from the system (J or kJ) m = mass of the substance (g) v = volume of the substance (L) c s = specific heat capacity (J / g o C ) c v = volumetric heat capacity (KJ / L o C)  t = t final – t initial = change in temperature ( o C)

Main Formulas Enthalpy change can be calculated using the following: Enthalpy change can be calculated using the following:Equation:  H = n H or  H = m H  H = n H or  H = m H MWhere:  H = enthalpy (energy) change for the phase change (KJ) n = moles of the substance undergoing the phase change (mol) H = molar enthalpy for the substance undergoing the phase change (KJ / mol) from Table 10.3 p.347. m = mass of the substance undergoing the phase change (g) M = molar mass of the substance undergoing the phase change (g / mol)

Main Formulas Calculating total energy: Calculating total energy:  E tot = sum of the parts of the heating curve = a + b + c + d + e = q ice +  H fus + q water +  H vap + qsteam

Main Formulas  H system = - q calorimeter  H system = - q calorimeter

Problems to Try…. When 150. L of water (in a hot water heater) at 10.0 o C is heated to 65.0 o C, how much energy is required? When 150. L of water (in a hot water heater) at 10.0 o C is heated to 65.0 o C, how much energy is required? If g of freon-12, CCl 2 F 2, was turned from a liquid to a gas at SATP, what is the expected enthalpy change,  H? If g of freon-12, CCl 2 F 2, was turned from a liquid to a gas at SATP, what is the expected enthalpy change,  H? Calculate the total energy released when 1.0 kg of molten iron, Fe (l), at 1700 o C, cools to solid iron, Fe (s), at 80 o C. The specific heat capacity of liquid iron is 0.20 J/g o C and that of solid iron is 0.11 J/g o C. The molar enthalpy of solidification of iron is -15 KJ/mol at 1535 o C. Calculate the total energy released when 1.0 kg of molten iron, Fe (l), at 1700 o C, cools to solid iron, Fe (s), at 80 o C. The specific heat capacity of liquid iron is 0.20 J/g o C and that of solid iron is 0.11 J/g o C. The molar enthalpy of solidification of iron is -15 KJ/mol at 1535 o C.

Problems to Try…. In a calorimetry experiment, 4.24 g of lithium chloride is dissolved in 100 mL of water at an initial temperature of 16.3 o C. The final temperature of the solution is 25.1 o C. Calculate the molar enthalpy of solution for lithium chloride In a calorimetry experiment, 4.24 g of lithium chloride is dissolved in 100 mL of water at an initial temperature of 16.3 o C. The final temperature of the solution is 25.1 o C. Calculate the molar enthalpy of solution for lithium chloride

Chemistry 122 Review Chapter 14

Vocabulary: equilibrium, Le Chatelier’s Principle Vocabulary: equilibrium, Le Chatelier’s Principle Types of changes: Types of changes: –concentration –temperature –pressure/volume (gases only)

Concentration changes addition of reactant  shifts equilibrium to the RIGHT addition of reactant  shifts equilibrium to the RIGHT removal of product  shifts equilibrium to the RIGHT removal of product  shifts equilibrium to the RIGHT addition of product  shifts equilibrium to the LEFT addition of product  shifts equilibrium to the LEFT removal of reactant  shifts equilibrium to the LEFT removal of reactant  shifts equilibrium to the LEFT Example : CaCO 3 (s)CaO (s) + CO 2 (g) + heat Example : CaCO 3 (s)CaO (s) + CO 2 (g) + heat What will happen to the equilibrium reaction above if: What will happen to the equilibrium reaction above if: –the concentration of CaCO 3 increases? SHIFT RIGHT to decrease concentration of CaCO 3 SHIFT RIGHT to decrease concentration of CaCO 3 –the concentration of CaCO 3 decreases? SHIFT LEFT to increase concentration of CaCO 3 SHIFT LEFT to increase concentration of CaCO 3 –the concentration of CaO (or CO 2 ) increases? SHIFT LEFT to decrease concentration of CaO (or CO 2 ) SHIFT LEFT to decrease concentration of CaO (or CO 2 ) –the concentration of CaO (or CO 2 ) decreases? SHIFT RIGHT to increase concentration of CaO (or CO 2 ) SHIFT RIGHT to increase concentration of CaO (or CO 2 )

Temperature changes Heat energy is treated as though it were a reactant or product Heat energy is treated as though it were a reactant or product Heat is added by heating and removed by cooling the container Heat is added by heating and removed by cooling the container reactants + energy products ENDOTHERMIC reactants + energy products ENDOTHERMIC reactantsproducts + energy EXOTHERMIC reactantsproducts + energy EXOTHERMIC Example : Example : 2 NaCl (s) + H 2 SO 4 (l) + energy 2 HCl (g) + Na 2 SO 4(s) 2 NaCl (s) + H 2 SO 4 (l) + energy 2 HCl (g) + Na 2 SO 4(s) What will happen to the equilibrium reaction above if: What will happen to the equilibrium reaction above if: –the reaction vessel is heated? SHIFT RIGHT to decrease energy on reactants side SHIFT RIGHT to decrease energy on reactants side –the reaction vessel is cooled? SHIFT LEFT to increase energy on reactants side SHIFT LEFT to increase energy on reactants side

Pressure/volume changes only affects systems involving gases only affects systems involving gases consider: the total amount in moles of gas reactants and the total amount in moles of gas products consider: the total amount in moles of gas reactants and the total amount in moles of gas products if # moles of gas reactants = # moles of gas products : if # moles of gas reactants = # moles of gas products : –no affect on equilibrium if # moles of gas reactants  # moles of gas products: if # moles of gas reactants  # moles of gas products: –an increase in pressure (decrease in volume) will shift equilibrium to the side with fewer moles of gas –a decrease in pressure (increase in volume) will shift equilibrium to side with more moles of gas

Pressure/volume changes Example: Example: 2 SO 2 (g) + O 2 (g) 2 SO 3 (g) + energy 2 SO 2 (g) + O 2 (g) 2 SO 3 (g) + energy # moles of gas reactants # moles of gas products # moles of gas reactants # moles of gas products = 3 = 2 = 3 = 2 What will happen to the equilibrium reaction above if: What will happen to the equilibrium reaction above if: –the pressure inside the reaction vessel increases? SHIFT RIGHT to side with less moles of gas (products) SHIFT RIGHT to side with less moles of gas (products) –The pressure inside the reaction vessel decreases? SHIFT LEFT to side with more moles of gas (reactants) SHIFT LEFT to side with more moles of gas (reactants)

Example Given: Given: N 2 (g) + 3 H 2 (g) 2 NH 3 (g) + heat N 2 (g) + 3 H 2 (g) 2 NH 3 (g) + heat How will this equilibrium respond to the following changes? How will this equilibrium respond to the following changes? (a) A decrease in temperature? (a) A decrease in temperature? (b) A decrease in pressure? (b) A decrease in pressure? (c) An increase in nitrogen? (c) An increase in nitrogen? (d) A decrease in ammonia? (d) A decrease in ammonia? Answers: (a) RIGHT (b) LEFT (c) RIGHT (d) RIGHT

Chemistry 122 Review Chapter 7

Vocabulary Limiting reagent, excess reagent, gravimetric, solute, solvent Limiting reagent, excess reagent, gravimetric, solute, solvent

Steps to Stoichiometry Step 1: write a balanced chemical equation and list the measurement and conversion factors for the given and required substances Step 1: write a balanced chemical equation and list the measurement and conversion factors for the given and required substances Step 2: convert the given measurement to an amount in moles by using the appropriate conversion factor. Step 2: convert the given measurement to an amount in moles by using the appropriate conversion factor. Step 3: Calculate the amount of the required substance by using the mole ratio from the balanced equation Step 3: Calculate the amount of the required substance by using the mole ratio from the balanced equation Step 4: Convert the calculated amount to the final required quantity by using the appropriate conversion factor or the ideal gas law. Step 4: Convert the calculated amount to the final required quantity by using the appropriate conversion factor or the ideal gas law.

Try This….. If 300g of propane burns in a gas barbecue, what volume of oxygen at SATP is required for the reaction? If 300g of propane burns in a gas barbecue, what volume of oxygen at SATP is required for the reaction? Calculate the mass of lead (II) chloride precipitate produced when 2.57g of sodium chloride in solution reacts in a double replacement reaction with excess aqueous lead (II) nitrate. Calculate the mass of lead (II) chloride precipitate produced when 2.57g of sodium chloride in solution reacts in a double replacement reaction with excess aqueous lead (II) nitrate.

Exam Format Matching (definitions and structures) – 12 marks Matching (definitions and structures) – 12 marks Definitions – 10 marks Definitions – 10 marks Organic naming and drawing structures – 30 marks Organic naming and drawing structures – 30 marks Calculations – 40 marks Calculations – 40 marks Short answer – 8 marks Short answer – 8 marks Total: 100 marks Total: 100 marks