Chapter 6- Thermochemistry Flashcards
Law of Conservation of Energy
energy can be transformed from one form to another, but it cannot be created or destroyed
Potential energy
energy due to position or composition
Kinetic energy (KE)
energy due to the motion of an object, depends on mass and velocity
KE Formula
KE=½mv^2
Temperature
property that reflects random motion of particles in a particular substance
Heat (q)
involves the transfer of energy between 2 objects due to difference in temperature
Work (w)
force acting over a distance
State Function
property of a system that depends only on its present state, and is independent of the particular pathway
Exothermic
chemical reaction that results in an evolution of heat, energy is flowing out of the system
Endothermic
chemical reaction that absorbs energy, and flows into the system
Endothermic
chemical reaction that absorbs energy, and flows into the system
Enthalpy (H)
property of a system that measures the system’s ability to allow heat or energy to flow through
Formula of enthalpy change
H=E+PV
+H, +q, +w, compressed gas, -volume
Reaction is endothermic
-H, -q, -w, expanding gas, +volume
Reaction is exothermic
Calorimetry
measuring heat and is based on observing temperature change
Heat Capacity (C) formula
heat absorbed /increase in temperature
Specific heat capacity (s)
energy required to heat 1g of a substance
Heat formula
q=smT
1st law of thermodynamics
energy of the universe is constant
Internal energy
the sum of the kinetic and potential energy of all particles in the system
Internal energy formula
E=q+w
Formula for work
w=-PV
1 L*atm=
101.325 J
