1. Chapter 11 Section 1 Thermochemistry -study of heat changes that occur during chemical reactions energy- ability to do work or supply heat -unlike matter, energy is weightless, odorless, tasteless -only way to detect energy is by its effects ex- gas in a car produces moving car when ignited

2. work- done when a force moves an object potential energy(PE)- energy of position, stored energy Ex- gas in car kinetic energy(KE)- energy of motion -faster = more kinetic energy Ex- car moving after being started

3. Law of Conservation of Energy -energy can neither be created nor destroyed -energy can be transferred from one object to another and from one form to another heat- flow of energy from one object to another because of a temperature difference *will be transferred until equilibrium is reached *transferred from warmer to cooler

4. All chemical reactions involve the release or absorption of heat: system- what is being studied surroundings- everything else around the system in nature universe- system and surroundings together *the system either loses energy to or gains energy from the surroundings

5. Heat Flow → two directions 1)surroundings → system endothermic- system gains heat as surroundings cool, system absorbs heat Ex- people (system) around a campfire 2)system → surroundings exothermic- system loses heat as surroundings heat up, system releases heat Ex- campfire (system)

6. Units of Energy joule(J) - SI unit for heat/energy -can use kJ1kJ = 1000J calorie(cal) - amount of energy required to raise the temp of 1g of pure water 1°C Calorie(Cal) - nutritional unit **1Cal = 1kcal = 1000cal **1J = 0.2390 cal4.184J = 1cal

7. Convert: 1)1656.70J → cal 1656.70 x 0.2390 or 1656.70/4.184 395.95cal or 395.96cal 2) 483.12cal → J 483.12/0.2390 or 483.12 x 4.184 2021.42J or 2021.37J 3) 0.56721Cal → J 0.56721 x 1000/0.2390 or 0.56721 x 1000 x 4.184 2373.26J or 2373.21J

8. heat capacity - the quantity of heat required to change the temperature of a system 1°C specific heat capacity- the amount of heat needed to raise the temperature of 1g of a substance by 1°C -the higher the specific heat capacity, the more energy is required to raise the temperature ex- water -metals tend to have fairly low specific heats because they heat up easily

9. Specific heat of water = 4.18 J/g°C q = (m)(C)(ΔT) q = heat (J or cal) m = mass (g) C = specific heat capacity (J/g°C) *will be given to you if not solving for- page296 ΔT = temp change T final – T initial (°C) m = q/C∆T C = q/m∆T ∆T = q/mC