Thermochemistry. Thermodynamics Study of energy transformations Thermochemistry is a branch of...
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Transcript of Thermochemistry. Thermodynamics Study of energy transformations Thermochemistry is a branch of...
Thermochemistry
Thermodynamics
Study of energy transformations Thermochemistry is a branch of
thermodynamics which describes energy relationships in chemical reactions
Energy
Capacity to do work or to transfer heat Mechanical work (w) is the product of force (F)
operating on an object and the distance (d) through which it moves
W = F x d Energy is required to do work
Heat (Q)
Heat is the energy transferred from one object to another due to a difference in temperature
Forms of Energy
Kinetic Energy – energy of motion- magnitude depends on the mass of the object and its velocity- EK = ½ m v2
- both mass and speed determine how work it can do
Potential Energy – stored energy Other forms of energy are simply types of
kinetic or potential on an atomic or molecular level
Energy Units
Joule (J) 1J = 1 kg m2/ s2
A calorie (cal) is the amount of energy required to raise the temp of 1 g of water 1 ºC
1 cal = 4.184 J
Example
A 145 g baseball is thrown with a speed of 25 m/s. Calculate the kinetic energy in Joules.
What is the kinetic energy in calories?
Systems
Portion we single out for study Surroundings is everything else outside the
system When studying energy changes in a chemical
reaction, the reactants and products are the system and everything else is the surroundings
Law of Conservation of Energy
Energy can be converted from one form to another but cannot be created or destroyed
Also called “First Law of Thermodynamics”
Internal Energy
Total energy of a system – sum of kinetic and potential energies
Cannot determine exact internal energy Can only determine a change in internal
energy ΔE = Efinal – Einitial
If ΔE is positive there is a gain in internal energy in the system
If ΔE is negative the system lost energy to its surroundings
Higher energy systems tend to lose energy and are therefore less stable
Heat and Work
Any system can exchange energy with surroundings in two ways – as heat or work
Internal energy increases as heat is added to or work is done on a system
ΔE = Q + wQ is positive if heat is added to systemw is positive if work is done on the system
Heat Changes
Exothermic Reactions – when heat is given off by the reaction (-Q)
Endothermic Reactions – when heat is used by the reaction (+Q)
Example
As a combustion reaction occurs the system loses 550 J of heat to its surroundings and it does 240 J of work in moving a piston. What is the change in its internal energy?
State Function
These are systems for whom the value of ΔE does not depend on the previous history of the sample, only on the present condition
Energy is a state function Work and heat are not state functions