Unit 11 PowerPoint
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Transcript Unit 11 PowerPoint
Key Terms
Average kinetic energy - Energy associated with the movement of
matter and mass
Bond energy - The amount of energy it takes to break one mole of
bonds
Calorimetry - measurement of quantities of heat
Chemical energy - the energy in a substance that can be released by a
chemical reaction
Collision theory - explains how chemical reactions occur and why
reaction rates differ for different reactions
Delta H (ΔH) - a measure of the energy associated with a system
Endothermic - Requiring a net input of heat for its formation
Enthalpy - a measure of the energy associated with a system
Key Terms
Exothermic - Accompanied by the release of heat
Heat - a form of energy that is transferred by a difference in
temperature
Molecular movement - how molecules move and is measured by
temperature
Potential energy diagram - plots the change in potential energy that
occurs during a chemical reaction
Specific heat - The heat required to raise the temperature of the unit
mass of a given substance by a given amount
Temperature - The measure of molecular motion or the degree of heat
of a substance
Thermal energy - The total potential and kinetic energy associated
with the random motions of the molecules of a material
Types of Energy
Mechanical
Kinetic – based on particle motion
Potential – based on height and acceleration due to gravity
Chemical
Kinetic – based on particle motion to define temperature
Equation: KE=1/2 MV2
Potential – energy stored in chemical bonds
Electrical – based on the flow of electrons from an area of high charge to an area of low
charge
Nuclear – based on the release of energy stored in the nucleus
Thermal – based on the transfer of heat
Energy Transfer
Energy always flows from a position of high energy to a
position of low energy
There are multiple ways that energy is transferred
Potential to Kinetic as objects fall
Kinetic to potential as objects rise
Electrical
Chemical as reactions occur
Thermal from hot to cold (energy cannot be transferred
from cold to hot)
Chemical Energy Transfer
The chemical energy transferred in chemical reactions is related
to the difference in potential energy of the reactants and the
products
The potential energy of chemical compounds is stored in the
compounds when they are formed – the heat of formation (Hfo)
We standardize the heats of formation based on the difference
found when the compounds are formed from elements.
This means that the heat of formation of any element always
equals zero
Enthalpy & Types of Reactions
When thermal energy leaves the reaction, the reaction is called
exothermic
∆HRXN is negative – thermal energy is leaving the system
Potential energy of products is less than the potential energy of
the reactants
It is the excess potential energy of the reactants that is leaving as
thermal energy
When thermal energy comes into the reaction, the reaction is called
endothermic
∆HRXN is positive – thermal energy is entering the system
Potential energy of products is greater than the potential energy
of the reactants
It is the thermal energy entering the system that provides the
additional potential energy needed to form the products.
Reaction Coordinate Diagrams for
Endothermic & Exothermic Reactions
Energy of Reactants < Energy of Products
Energy of Products < Energy of Reactants
Endothermic
Exothermic
ΔHRXN = ΔHProducts - ΔHReactants
Heat of Reaction - Enthalpy
The heat transfer in a chemical reaction is defined as enthalpy which
represents the change in the energy stored in the chemical bonds
The Enthalpy is equal to the overall change in chemical potential
energy: ∆HRXN
Enthalpy = Potential Energy of Products – Potential Energy of
Reactants
∆HRXN = ∑ ∆Hf0 (products) - ∑ ∆Hf0 (reactants)
Law of Conservation of Energy
Energy may not be created or destroyed
Energy may change form
Therefore, the sum of all of the energies in a system is a constant
Enthalpy = Potential Energy of Products – Potential Energy of
Reactants
∆HRXN = ∑ ∆Hf0 (products) - ∑ ∆Hf0 (reactants)
∆HRXN is positive, the reaction is endothermic
∆HRXN is negative, the reaction is exothermic
Specific Heat & Calorimetry
The heat of reaction is measured through a process of
determining the effect on the environment.
Assuming no loss of energy, the energy out of one system
is equal to the gain in energy of another system.
Calorimetry is the process of quantifying this energy
Calorimetry is dependent on knowing the effect of
temperature change on the environment – specific heat
Specific Heat
Specific Heat (cp) - The amount of thermal energy (heat)
required to change the temperature of one gram of matter, one
degree Celsius.
The use of specific heat allows for determining the amount of
heat lost or gained.
Heat gained or lost = (mass) (specific heat) (change in temperature)
q = m cp ΔT
Heating Curve of Water
Image used courtesy of http://ch301.cm.utexas.edu/thermo/selector.php?name=heat-curves
Calorimetry
Assuming no loss of heat, the thermal energy out of one
system is equal to the gain in thermal energy of another
system.
qin = - qout
If qout = ∆HRXN , then
qin = - ∆HRXN
If enthalpy is negative, temperature increases (exothermic)
If enthalpy is positive, temperature decreases (endothermic)