Heat in Chemical Reactions - PowerPoint PPT Presentation

1 / 25
About This Presentation
Title:

Heat in Chemical Reactions

Description:

Heat in Chemical Reactions 10.1 Chemical Reactions that Involve Heat Heat: Energy (symbol - q) that is transferred from one object to another due to a ... – PowerPoint PPT presentation

Number of Views:79
Avg rating:3.0/5.0
Slides: 26
Provided by: Groa152
Category:

less

Transcript and Presenter's Notes

Title: Heat in Chemical Reactions


1
Heat in Chemical
Reactions
2
10.1 Chemical Reactions that Involve Heat
  • Heat Energy (symbol - q) that is transferred
    from one object to another due to a difference in
    temperature. Measured in Joules (symbol - J)
  • 2. Thermochemistry The study of heat changes in
    a chemical reaction.

3
3. Types of Chemical Reactions
  • a. Exothermic Reactions release heat into their
    surroundings. Heat is a product of the reaction
    and temperature increases. This occurs during
    bond formation.
  • Combustion reactions are exothermic burning
    propane
  • C3H8 5O2 ? 3CO2 4H2O 2043 kJ

surroundings
Exothermic Reaction
?T
?H -
4
Exothermic Reaction
5
  • b. Endothermic Reactions Heat is absorbed by the
    reactants and stored in the chemical bonds of the
    products. Heat acts as a reactant and
    temperature decreases. This occurs during bond
    breaking.
  • Electrolysis of water requires electrical energy.
  • 2H2O 572kJ ? 2H2 O2

surroundings
Endothermic Reaction
?T -
?H
6
Exothermic/Endothermic Reactions
7
10.2 Heat and Enthalpy Changes
  • 1. Enthalpy The heat content of a system at
    constant pressure (symbol is H ).
  • 2. Enthalpy Change The heat absorbed or released
    during a reaction (symbol is ?H ).
  • SKIP TO TOP of PAGE 3

8
  • 4. When reactions take place at standard
    temperature and pressure, q H.
  • 5. Standard Enthalpy Change (?H?) Enthalpy
    change that occurs when reactants in their
    standard states (most stable form) change to
    products in their standard states. STP Standard
    Temperature and Pressure are 0 ?C and 1 atm.
  • The ?H? is listed after the equation. If the
    ?H? is positive the reaction is endothermic and
    heat was absorbed. If the ?H? is negative, the
    reaction is exothermic and heat was released.
  • 6. The amount of heat absorbed or released in a
    reaction depends upon the number of moles of
    reactants.

9
7. Enthalpy Changes in Stoichiometry Problems
  • Ex) How much heat will be released if 5.0 g of
    H2O2 decomposes?
  • 2H2O2 ? 2H2O O2 ?H? -190 kJ

10
  • Ex) How much heat is transferred when you eat a
    10. g Jolly rancher which is made of glucose
    (C6H12O6)? It reacts in your body with oxygen
    according to the following equation. If 4.184kJ
    1 Cal, how many Calories are in the Jolly
    Rancher?
  • C6H12O6 6O2 ? 6CO2 6H2O ?H? -2803 kJ

C6H12O6 6O2 ? 6CO2 6H2O 2803 kJ
11
3. Enthalpy Diagrams 1 2
12
1 2
a. Which has a higher enthalpy? Products or Reactants R P
b. Was heat absorbed or released? R A
c. Is this an endothermic or exothermic reaction? Exo Endo
d. Is ?H for this reaction positive or negative? -
e. Would the ?H be on the left or right side of the yield sign? R L
f. Is the reverse reaction exothermic or endothermic? Endo Exo
13
g. Rewrite each equation with the heat term in
the reaction as a reactant or product
  • 1) C3H8 5O2 ? 3CO2 4H2O 2043 kJ
  • 2) C H2O 113kJ ? CO H2

14
? change in ?H Hproducts - Hreactants
?H Hproducts Hreactants
Exothermic Reaction - low high
Endothermic Reaction high low
15
10.3 Hesss Law - (1802-1850)
  • The enthalpy change for a reaction is the sum of
    the enthalpy changes for a series of reactions
    that adds up to the overall reaction.
  • This is also called the Law of Heat of Summation
    (S)
  • 3. This allows you to determine the enthalpy
    change for a reaction by indirect means when a
    direct method cannot be done.

16
4. Steps for using Hesss Law
  • 1. Identify the compounds
  • 2. Locate the compounds on the Heat of Reaction
    Table.
  • 3. Write the reaction from the table so the
    compound is a reactant or product.
  • 4. Write appropriate ?H for each sub equation.
  • If needed, multiply equation and enthalpy change
    value. (coefficients)
  • If you reverse the equation, change the sign of
    the enthalpy change.
  • 5. Add the equations to arrive at the desired net
    (original) equation.
  • 6. Add ?H (enthalpy changes) of each sub
    equation.

17
10.3 Calorimetry
  • 1. The Kinetic Theory states that heat results
    from the motion vibration of particles.
  • 2. Heat The transfer of kinetic energy from a
    hotter object to a colder object. Heat is
    dependent on composition and amount.
  • 3. Temperature is a measure of how hot or cold
    something is specifically it is the measure of
    the average kinetic energy (speed) of the
    particles in an object. It is independent of
    amount.

18
Heat
  • Temperature is not the same as heat.
  • Temperature is a measure of the average kinetic
    energy of the particles in an object.
  • A temperature change is a result of a energy
    transfer.
  • Julius Sumner Miller - Physics - Heat
    Temperature
  • Heat vs. Temperature Animation

19
  • 4. Calorimetry is the study of heat flow and
    measurement.
  • 5. Calorimetry experiments determine the heats of
    reactions (enthalpy changes) by making accurate
    measurements of temperature changes produced in a
    calorimeter.
  • 6. A Calorimeter is an insulated device used to
    measure heat absorbed or released in a chemical
    or physical change.

20
  • 7. Specific Heat (Cp) The amount of heat needed
    to raise 1 g of a substance by 1?C.
  • Formula for specific heat
  • mmass (substance)
  • ?Tchange in temperature of the substance (Tf-Ti)
  • Specific Heat of Water 4.184 J/g ºC
  • 1 calorie or .001food Calorie

21
  • 8. Measuring Specific Heat of a Metal
  • Ex 1) What is the specific heat of a nickel if
    the temperature of a 32.2 g sample of nickel is
    increased by 3.5ºC when 50. J of heat is added.

22
  • Ex 2) How much heat is absorbed to be able to
    increase the temperature of a 26.2 g sample of
    aluminum (Cp 0.897 J/gºC) from 25.3 ºC to 65.9
    ºC?

23
  • 9. Measuring Heat (q) of a Substance Dissolved in
    Water
  • You can rearrange this formula to determine
    the heat released or absorbed by the surroundings
    (solution) as the substance dissolves based on
    this assumption
  • q reaction -q surroundings
  • ?q
  • 1) Calculate q for the surroundings (solution)
    and determine qrxn.
  • 2) Calculate the moles of solute dissolved in the
    water.
  • 3) Calculate ?H

?T Tf - Ti
24
  • Ex) When a 4.25 g sample of solid NH4NO3
    dissolves in 60.0 g of H2O in a calorimeter,the
    temperature drops from 21.0 ºC to 16.9 ºC.
    Calculate ?H. Rewrite the thermochemical
    equation with the heat term as a reactant or
    product.
  • NH4NO3(s) ? NH4(aq) NO3-(aq) ?H
    ?
  • qsurmCp?T (64.3g)(4.184J/gC)(-4.1C)
  • qsur-1100J
  • qrxn -qsur 1100J
  • 2.
  • 3.

21 kJ
25
10. Foods as Fuels
  • A. Carbohydrates typically have high enthalpies
    however, the products of their combustion, CO2
    and H2O, have low enthalpies.
  • B. Therefore, the combustion of carbohydrates and
    fats, is exothermic.
  • C. Sugars and Starches break down to glucose,
    which reacts with O2 in a combustion reaction.
  • D. Nutritional information on food labels can be
    gathered using a calorimeter.
  • Carbs 4 Cal/g Protein 4 Cal/g Fat 9 Cal/g
Write a Comment
User Comments (0)
About PowerShow.com