Thermochemisrty Flashcards
(31 cards)
Specific heat capacity
Amount of heat needed to raise temp of 1 gram of a substance by 1 degree
Heat capacity
Amount of heat needed to raise the temp of an object by 1 degree
Specific heat capacity for water
4.186J/g degree Celsius
heats up slow
Specific heat capacity for lead
0.128J/g degree Celsius
Heats up fast
Heat absorbed by water
Q=mc
Heat of combustion
Energy released as heat when compound undergoes complete combustion with O under standard conditions
Endothermic
Reactant+reactant+ENERGY
=product+product
Exothermic
Reactant+reactant=product+product+ ENERGY
Isolated environment
Used to accurately determine how much thermal energy is produced in a combustion reaction
Open system
Can exchange both energy and matter with its strong surroundings
Closed system
No matter can enter or leave
Energy may be exchanged
Isolated system
No energy or matter can enter or leave
Bomb calorimeter
Isolated system
Molar enthalpy
Amount of energy released/ mole
Molar enthalpy equation
Chemical systems contain both _____ And _______ energy
Kinetic and potential
Enthalpy change
Energy absorbed from or released to the surroundings when a system changes from reaction to products
Enthalpy change equation
+or- lQsurroundingsl
Molar enthalpy
Enthalpy change per mile of a substance undergoing a change
Types of reactions
Solution Combustion Vaporization Freezing Neutralization Formation
Way to illustrate enthalpy change
Thermochemical equations
Thermochemical equations with energy terms
Exothermic (-) value goes on PRODUCT side
Endothermic (+) value goes on REACTANT side
Thermochemical equations with
Write balanced equation with
Molar enthalpies of reaction
Write down energy associates with the reaction of one mile of a substance
