Created by Lynne Crandall University of Michigan Revised by Mark Kondrak CLA Language Center University of Minnesota Could you put an image here?

Slides:



Advertisements
Similar presentations
Click a hyperlink or folder tab to view the corresponding slides.
Advertisements

Energy and Chemical Change
Thermodynamics Energy and Heat.
Chapter 6 THERMOCHEMISTRY West Valley High School AP Chemistry Mr. Mata.
CHAPTER 17 THERMOCHEMISTRY.
 Section 1 – Thermochemistry  Section 2 – Driving Force of Reactions.
Thermochemistry.  What is energy?  Energy is the ability to do work or produce heat.  The Law of Conservation of Energy: ◦ This law states that can.
Energy Transformations Thermochemistry is the study of energy changes that occur during chemical reactions and changes in state. The energy stored in the.
Chapter 17 Energy and Rate of Reactions.  Thermochemistry – study of the transfer of energy as heat that accompanies chemical reactions and changes 
Chapter 16 Reaction Energy
CHEMISTRY Matter and Change
 Section 1 – Thermochemistry  Section 2 – Driving Force of Reactions.
Energy Chapter 16.
Reaction Energy and Reaction Kinetics Thermochemistry.
Energy and Chemical Change
Unit 7 Review Game Board
Chapter 17 Thermochemistry.
1) vocab word--the quantity of heat needed to raise the temperature of 1 g of water 1°C 2) vocab word--the amount of energy required to raise the temperature.
ENERGY. Energy Review Temperature – measurement of the random motion of the components of a substance Heat – flow of energy due to temperature differences.
Thermochemistry. The study of heat changes in chemical reactions Exothermic: reactions that release heat Endothermic: reactions that absorb heat Enthalpy:
Back Chapter 17: Energy and Kinetics Thermochemistry: Causes of change in systems Kinetics: Rate of reaction progress (speed) Heat, Energy, and Temperature.
Section 18.4 Entropy. What you need to know - Entropy -Gibbs Free Energy -Enthalpy -Calculating Gibbs Free Energy -Determine if a rxn is spontaneous or.
Thermochemistry.  What is energy?  Energy is the ability to do work or produce heat.  The Law of Conservation of Energy: ◦ This law states that can.
Topic: Thermodynamics Do Now: packet p.1. Every physical or chemical change is accompanied by energy change  Energy released = _________________  Energy.
CHAPTER 16: SPONTANEITY, ENTROPY, & FREE ENERGY Dr. Aimée Tomlinson Chem 1212.
Thermodymanics.  Thermodynamics is a branch of science that focuses on energy changes that accompany chemical and physical changes.
Chapter 17 Energy and Chemical Change. Thermochemistry The study of heat changes in chemical reactions.
Thermochemistry, Hess’s Law and Driving Forces Review p Define: temperature, heat, specific heat, calorie and joule, exothermic, endothermic,
Unit 13: Thermochemistry Chapter 17 By: Jennie Borders.
Thermochemistry! AP Chapter 5. Temperature vs. Heat Temperature is the average kinetic energy of the particles in a substance. Heat is the energy that.
THERMOCHEMISTRY.
$$$ Quiz $$$ Thermochemistry. Gives off heat (emits) exothermic.
THERMOCHEMISTRY. Definitions #1 Energy: The capacity to do work or produce heat Potential Energy: Energy due to position or composition Kinetic Energy:
Chapter 15 Energy and Chemical Change Energy Energy can change for and flow, but it is always conserved.
Thermochemistry Energy Heat Thermochemical Equations Calculating Enthalpy Change Reaction Sponteneity.
Thermodynamics Thermochemistry Carol Brown Saint Mary’s Hall.
Ch. 11 Thermochemistry: Heat and Chemical Change
 Section 1 – Thermochemistry  Section 2 – Driving Force of Reactions.
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.
 What is the formula for finding heat?  What are the two units of heat?  The temperature of a sample of iron with a mass of 10.0 g changed from 50.4.
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.
THERMOCHEMISTRY. Definitions #1 Energy: The capacity to do work or produce heat Potential Energy: Energy due to position or composition Kinetic Energy:
Unit 11 Thermodynamics Chapter 16. Thermodynamics Definition Definition A study of heat transfer that accompanies chemical changes A study of heat transfer.
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.
THERMOCHEMISTRY. Definitions #1 Energy: The capacity to do work or produce heat Potential Energy: Energy due to position or composition Kinetic Energy:
Thermochemistry Thermochemistry is the study of the transfers of energy as heat that accompany chemical reactions and physical changes.
Enthalpy, Entropy, and Spontaneity Explained. Review of Enthalpy Change.
 Energy – the ability to do work or produce heat ◦ Kinetic energy – energy of motion ◦ Potential energy – stored energy  Chemical potential energy –
Thermodynamics Cartoon courtesy of NearingZero.net.
Energy & Heat Energy – ability to produce heat Heat - energy in the process of flowing from a warmer object to a cooler object. In chemical reactions.
Thermochemistry Some Like It Hot!!!!!. The Flow of Energy ► Thermochemistry – concerned with heat changes that occur during chemical reactions ► Energy.
THERMOCHEMISTRY. Definitions #1 Energy: The capacity to do work or produce heat Potential Energy: Energy due to position or composition Kinetic Energy:
THERMOCHEMISTRY. Definitions #1 Energy: The capacity to do work or produce heat Potential Energy: Energy due to position or composition Kinetic Energy:
Energy change that occurs during a chemical reaction and/or changes in state.
Chapter 11 Thermo chemistry Heat and Chemical Change The Flow of Energy – Heat Measuring and Expressing Heat Changes Heat in Changes of State Calculating.
THERMOCHEMISTRY. Definitions #1 Energy: The capacity to do work or produce heat Potential Energy: Energy due to position or composition Kinetic Energy:
Section 15-5 Section 15.5 Reaction Spontaneity Differentiate between spontaneous and nonspontaneous processes. vaporization: the energy-requiring process.
CHEMISTRY – UNIT 12 Thermochemistry. Energy Energy – ability to do work or produce heat  Potential energy – energy due to composition or position of.
Ch. 16 Reaction Energy. Thermochemistry  Thermochemistry: the study of the transfers of energy as heat that accompany chemical reactions and physical.
Thermochemistry Energy and Chemical Change. Energy Energy can change for and flow, but it is always conserved.
Energy change that occurs during a chemical reaction and/or changes in state.
Chapter 15 Energy and Chemical Change Section 15.1 Energy Section 15.2Heat Section 15.3Thermochemical Equations Section 15.4 Calculating Enthalpy Change.
Thermochemistry Thermo = heat Chemistry = study of matter.
Unit 12 Thermodynamics Chapter 16. Thermodynamics Definition A study of heat transfer that accompanies chemical changes Concerned with overall chemical.
ENERGY OF REACTIONS Entropy, Enthalpy, and Gibb’s Free Energy.
Thermochemistry.
Energy and Chemical Change
You must turn in your notes
CHEMISTRY Matter and Change
Thermochemistry Chapter 16.
Presentation transcript:

Created by Lynne Crandall University of Michigan Revised by Mark Kondrak CLA Language Center University of Minnesota Could you put an image here?

ThermochemistryConceptsDefinitions Free energy, Enthalpy and Entropy Calculations Bring the heat

Categories A g piece of iron absorbs joules of energy, and its temperature changes from 25 o C to 175 o C. Calculate the specific heat capacity of iron. Calculations 100 pts

Categories Calculations 100 Points 0.46 J/(g o C)

Categories Calculations 200 Points If a reaction has a ∆H rxn of -700 kJ and a ∆S of J/K, What is ∆G rxn at 325 K?

Categories -80 kJ Calculations 200 Points

Categories Calculations 300 Points What is ∆H for the following reaction? 2CO (g) + 2NO (g)  2CO 2 (g) +N 2 (g) a.2CO (g) + O 2 (g)  2CO 2 (g) ∆H= kJ b. N 2 (g) + O 2 (g)  2NO (g) ∆H = kJ

Categories Calculations 300 Points kJ

Categories Use the standard enthalpies of formation to calculate ∆H rxn, for the combustion of methane. ∆H o f (CO 2) = -394 kJ ∆H o f (H 2 O) = -286 kJ ∆H o f (CH 4 ) = -75 kJ Calculations 400 Points

Categories ∆H o rxn = -891 kJ Calculations 400 Points

Categories Consider the reaction below at 25 o C for which ∆S= 16.1 J/K and ∆H=163.8 kJ. CH 4 (g) + N 2 (g)  HCN (g) + NH 3 (g) At what temperature will this reaction be spontaneous? Calculations 500 Points

Categories Above K Calculations 500 Points

Categories The amount of energy absorbed by a substance to change it from a liquid to a gas Bring the Heat 100 Points

Categories Bring the Heat 100 Points What is heat of vaporization?

Categories Bring the Heat 200 Points The amount of energy absorbed by a substance to change from a solid to a liquid.

Categories What is heat of fusion? Bring the Heat 200 Points

Categories At constant pressure, q=? Bring the Heat 300 Points

Categories ∆H rxn Bring the Heat 300 Points

Categories Bring the Heat 400 Points The amount of heat required to raise the temperature of one gram of pure water by one degree Celsius.

Categories Bring the Heat 400 Points What is a calorie?

Categories ∆H fusion is a(n) ______________ reaction. Bring the Heat 500 Points

Categories Endothermic Bring the Heat 500 Points

Categories The heat content of a system at constant pressure. Free Energy, Enthalpy and Entropy 100 Points

Categories Free Energy, Enthalpy and Entropy 100 Points What is enthalpy (H)?

Categories Free Energy, Enthalpy and Entropy 200 Points The energy available to do work.

Categories What is Gibbs Free energy (G)? Free Energy, Enthalpy and Entropy 200 Points

Categories Free Energy, Enthalpy and Entropy 300 Points A reaction is spontaneous when Gibbs Free energy is ____________.

Categories Free Energy, Enthalpy and Entropy 300 Points Negative

Categories Arrange the following in order of INCREASING entropy: S liquid, S gas, S solid Free Energy, Enthalpy and Entropy 400 Points

Categories S solid < S liquid < S gas Free Energy, Enthalpy and Entropy 400 Points

Categories When a reaction is endothermic and has decreasing entropy it is: a.Always spontaneous b.Never spontaneous c.Sometimes spontaneous Free Energy, Enthalpy and Entropy 500 Points

Categories Never spontaneous Free Energy, Enthalpy and Entropy 500 Points

Categories The ability to do work or produce heat. Definitions 100 Points

Categories Definitions 100 Points What is energy?

Categories Definitions 200 Points The process of energy flowing from a warmer object to a cooler object.

Categories What is heat? Definitions 200 Points

Categories Definitions 300 Points The measure of disorder or randomness in a system.

Categories Definitions 300 Points What is entropy?

Categories The change in enthalpy that accomapnies the formation of one mole of the compound in its standard state from its constituent elements in their standard states. Definitions 400 Points

Categories What is the standard enthalpy (heat) of formation? Definitions 400 Points

Categories The part of the universe that we are interested in studying. Definitions 500 Points

Categories What is the system? Definitions 500 Points

Categories What is the difference between an exothermic and endothermic reaction? Thermochemistry Concepts 100 Points

Categories Thermochemistry Concepts 100 Points An exothermic reaction releases heat while an endothermic reaction absorbs heat.

Categories Thermochemistry Concepts 200 Points Explain why a gaseous state of a substance has a greater entropy than the liquid state of the same substance.

Categories A gaseous substance has more disorder than a liquid substance because the particles are moving in a constant random motion. Thermochemistry Concepts 200 Points

Categories Thermochemistry Concepts 300 Points What is the equation for ΔH o rxn ?

Categories Thermochemistry Concepts 300 Points ΔH o rxn = ΣnΔH o f (products) - ΣnΔH o f (reactants)

Categories Thermochemistry Concepts 400 Points What is specific heat?

Categories Thermochemistry Concepts 400 Points The amount of heat required to raise the temperature of one gram of that substance by one degree Celsius.

Categories On the scale of standard enthalpies of formation, how are the elements in their standard states defined? Thermochemistry Concepts 500 Points

Categories Elements in their standard states are assigned enthalpies of formation of 0.0 kJ. Thermochemistry Concepts 500 Points

Categories

The Daily Double