Kinetics Flashcards
Ist Law of Thermodynamics
Energy can’t be created or destroyed, it can only be converted from one form to another
Potential energy
stored within the bonds
Kinetic energy
In the particles, they are always moving
Specific heat capacity vs. heat capacity
Specific - heat needed to increase the temp of a unit mass of material by 1K (J/g degree C)
heat needed to increase the temp of an object by 1K (J/degree C)
How does specific heat capacity differ from heat capacity
Specific heat of H20 is the same no matter the mass, heat capacity of pool is greater than a pot of water
positive delta H (enthalpy)
endothermic
negative delta H (enthalpy)
exothermic
Ea
activation energy
What is the amount of heat gained/lost based on
When the rxn is done - LA is used
Combustion
Burning produces heat
CO2 + H2O (O2 in excess)
CO + H2O (O2 limited)
Error in calorimetry
Some heat might be lost to the air or calorimeter, the measurements of the mass have fewer sig figs.
deltaH^circle f
Enthalpy change associated with forming 1 mole of a cmpd from its elements in their standard states at standard conditions (298 K and 1 x 10^5 Pa)
percent error
Accepted - actual / accepted x 100
Hess’s Law
The enthalpy change for any chemical rxn is independent of the route, provided that starting conditions, final conditions, reactants and products are the same.
Bond enthalpy
Energy needed to break 1 mole of bonds in gaseous molecules under standard conditions
