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THERMOCHEMISTRY, is, is, Figure 2.image, Figure 3.image, image, Figure 1.…
THERMOCHEMISTRY
Temperature
Measure of the average kinetic energy of the atoms or molecules in the system
Surrounding
is
everything else in the universe around the system
Heat (q)
Internal energy
is
Energy produced by the bonds between atoms in a molecule (motion of molecules)
composed by
Kinetic Energy
: motion of particles in an object
Translational kinetic energy: movement of the single atom by itself (linear movement)
Rotational and vibrational kinetic energy: movement between bonds
Potential Energy
: attraction between the particles
produced by
Intermolecular forces: produced by the interation between molecules
Dipole-dipole forces (interaction between polar molecules)
Hydrogen bonds (interaction between a Hydrogen atom + electronegative atom)
London forces (interacion between non-polar molecules)
energy contained within a system because of its position
Process in which thermal energy is transferred from a hotter system to a cooler system that are in contact
Specific Heat
is
Energy required to increase in 1 °C the temperature of 1 gram of susbstance
example:
It takes less energy to raise the temperature of 1 gram of lead by 1°C than to raise the temperature of 1 gram of water by 1°C.
because
Energy in the lead spreads quickly as the temperature goes up
particles are closer
vibrate faster
Water has a higher internal energy
and
It needs more energy to break hydrogen bonds between molecules
Studies the importance of energy in chemical reactions
Energy
Capacity to do work
Law of Conservation of Energy
energy can't be created nor destroyed
System
is
where the chemical reaction is taking place
Enthalpy
(H)
is
Amount of energy a reactant has to lose/gain to create a product
It's only posible to measure the enthalpy change
the system moves from an initial state to a final state
Enthalpy change
(ΔH)
is
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is
is
Figure 2.
Figure 3.
Figure 1. Internal energy of systems with the same temperature:
Figure 4.1
Figure 4.2
Figure 4.3
is
states that
Figure 5.
Figure 6. Specific heat of certain substances:
as
Figure 7.
Figure 8.
Figure 10.2 Enthalpy Level Diagram: Exothermic reactions
Figure 9.1
Figure 11.2 Enthalpy Level Diagram: Endothermic reactions
Figure 9.2
Figure 9.3
Figure 10.1 Example:
Figure 11.1 Example:
