1. Energy Flow

2. Energy the ability to do work energy has no mass nor volume but is only detected by its effects thermochemistry studies energy changes during chemical reactions and state changes chemical potential energy is the energy stored in chemical bonds

3. Heat (q) energy that transfers from one object to another  moves from hot to cold  no such thing as cold (only the absence of heat) the term “universe” is…  system- part you focus on  surrounding- everything else/outside  energy is conserved so that all energy of the “universe” remains unchanged (law of conservation of energy) http://search.live.com/images/results.aspx?q=thermochemistry&form=QBIR#focal =f63acfb36eecbdd0428d134cb42a44ea&furl=http%3A%2F%2Fhighered.mcgraw- hill.com%2Fsites%2Fdl%2Ffree%2F0072512644%2F117362%2F06_p239bottom.j pg

4. Direction of Heat Flow Endothermic system gains heat as the surrounding cools down positive q

5. Exothermic system loses heat as the surrounding heats up negative q

6. Measuring Heat (not temp.) use the calorie (cal) or joule (J) 1 cal is the quantity of heat needed to raise 1 g of pure water, 1ºC in foods, one Calorie is equal to 1000 calories 41 Calories in a candy bar means that when burned, it will release 41 Calories (41,000 calories)

7. Heat Capacity and Specific Heat heat capacity depends on object’s mass and chemical compostion amount of heat needed in increase an object 1ºC specific heat depends on chemical composition and mass is held constant (1 gram) the amount of heat needed to increase 1 gram of a substance 1ºC

9. q m · ΔT q = heat (in joules or calories) m = mass (g) ΔT = change in temperature (ºC) C = specific heat (J/g·ºC) or (cal/g·ºC) C =

10. What is the specific heat of a substance that absorbs 2500 joules of heat when a sample of 10,000 g of the substance increases in temperature from 10.0ºC to 70.0ºC? 2500 J 10,000 g (60ºC) = 0.0042 J/g·C C =

11. The specific heat of ethanol is 2.46 J/g· o C. Find the heat energy required to raise the temperature of 193 g of ethanol from 19 o C to 35 o C q 193 g (16 o C) q = + 7600 J 2.46 J/g· o C =

12. Hard problem A 25 g sample of iron (initially at 800.00 o C) is dropped into 200 g of water (initially at 30.00 o C). The final temperature of the system is 40.22 o C. Find the specific heat of iron. (Specific heat of water is 4.18 J/g· o C) = 0.45 J/g o C