Chapter 11 Section 1 Thermochemistry -study of heat changes that occur during chemical reactions energy- ability to do work or supply heat -unlike matter,

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Presentation transcript:

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

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

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

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

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)

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 = cal4.184J = 1cal

Convert: 1) J → cal x or / cal or cal 2) cal → J / or x J or J 3) Cal → J x 1000/ or x 1000 x J or J

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

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

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