Equations
Practice Q's
Vocab
Vocab
100
The equation for specific heat
c=q/mΔT
100
______ Calorie = _____ kilocalories = 1000 calories
1Cal, 1000kcal
100
The study of energy changes that occur during chemical reactions and changes in states
thermochemistry
100
Heat absorbed by 1 mol of a solid substance as it melts to a liquid at constant temperature
heat of fusion
200
This equation calculates ΔH= Δproducts - Δ reactants
Calculating the change of enthalpy
200
Depends on mass and chemical properties
the heat capacity of an object
200
Energy stored in the chemical bonds of a substance
chemical potential energy
200
States that in any chemical or physical process energy is neither created nor destroyed
Law of conservation of energy
300
Endothermic or Exothermic? 1. Molar Heat of solidification = ΔHsolid: 2. Molar Heat of fusion = ΔHfus: 3. Molar Heat of vaporization = ΔHvap: 2. Molar Heat of condensation = ΔHcond:
1. Exothermic 2. Endothermic 3. Endothermic 4. Exothermic
300
It takes 487.5 J to heat 25 grams of copper from 25 °C to 75 °C. What is the specific heat in Joules/g·°C?
c = 487.5 J/(25g)(50 °C) c = 0.39 J/g·°C
300
________ process absorbs heat from the surroundings ________ releases heat into its surroundings
1. Endothermic 2. Exothermic
300
Law that states if you add two or more thermochemical equations to give a final equation then you can also add the heats of reactions to give the final heat of reaction.
Hess's Law of heat summation
400
If the specific heat is lower the less energy it takes to ...
Raise the temperature of a substance 1ºC
400
Find the mass of water than increases its temperature by 10°C and releases 1400 J of energy. Specific heat of water= 4.18 J/g·ºC
1400/(4.18*10) = 33.5 g
400
Heat of reaction for the complete burning of 1 mol of a substance
heat of combustion
400
amount of heat released when 1 mole of vapor condenses at the normal boiling point
molar heat of condensation
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