Thermochemistry Chapter 5 Regular Chem book = Ch 11

Hmmmmmm… When we eat calories where is the HEAT in food? What do we do with it (what do we convert it into) when we “burn” calories? Food’s heat is in its bonds- it’s energy is being used to hold the particles together We break the bonds and release that energy- then we convert it to movement and heat

Try this… Place a PEA-SIZED piece of anhydrous (aka dried out) CuSO 4 in your hand Add a few drops of water What do you feel? Wash your hands

Put the THERMO in Chemistry Mg + HCl  MgCl 2 + H 2 But, that’s only part of the story because this reaction gives off lots of heat! + heat That turns a chemical equation into a thermochemical equation

2 types: 1.Endothermic Reaction or process that __________ heat ΔH is Reactants have _____ heat than products absorbs positive less

2 types: 2.Exothermic Reaction or process that __________ heat ΔH is Reactants have _____ heat than products releases negative more

Exo and Endo (cont.) For every exothermic process, there’s an endothermic partner What’s exo/endo in… Freezing ice? Boiling water? BBQing sausages? You outside on a super cold day?

Thermo Equations There are 3 different ways to write a thermo equation: 1.H 2 O (l) + heat  H 2 O (g) 2.H 2 O (l)  H 2 O (g) ΔH= -285kJ 3. H 2 O (g) H 2 O (l)

Try it! 1 mole of ice needs to absorb 285kJ of heat in order to melt. Write the thermo equation 3 ways.

Try it! The combustion of methane releases 890kJ of heat. Write the equation for this reaction 3 ways. Wait, combustion releases heat but you have to add heat to make it happen. What’s up with that?

Heat? Measured in Calories 1 Cal = 1 kilocal or kcal = 1000 cal Joules J = 1 calorie 1000 J = 1 kJ

Thermo Stoich Calcs CaO + H 2 O  Ca(OH) kJ Which means that 1 mole of CaO produces 65.2kJ of heat …and that adds another arrow to the molar conversion map How much heat will 4 moles produce? How much will 100g produce? What mass of CaO is needed to make 1000kJ? Interesting little tidbit… this is the reaction when you make cement. You add little rocks and stuff to CaO and then add water. 4 x 65.2 = kJ 100/56 x 65.2 = kJ 1000/65.2 x 56 = 858.9g

Calculations Practice Fe 2 O 3 + 3CO  2Fe + 3CO kJ Is this exo or endothermic? How much heat would be produced from 1.2 moles of CO? How about from 100L of CO (at STP) Exothermic 1.2/3 x 26.3 = / 22.4 / 3 x 26.3 = 39.1kJ

Specific Heat So… you’re out walking barefoot on a 90 o day and you have the choice to step on (a) the sidewalk (b) a manhole cover (c) a puddle What would you do?

Specific Heat II (Specific) Heat capacity = the amount of heat it takes to raise 1g of a substance by 1 o C -- Water is high, metal is low -- What else is high & low? (p. 296) -- What’s up with the oranges on p. 297?

Specific Heat III q = mC Δ T q is the heat in cal or J m is the mass in g C is the specific heat in J/g o C or cal/g o C Δ T is the temp change in o C Try #1-3, on page 299

Calorimetry Method of measuring temperature change in order to calculate heat change Measure temp change of water* Use q=mC  T to find q… q absorbed by water= q released by reaction

q=mC Δ T Example #1: 94.6g of Cu heats up 25  40 o C by absorbing 849J, what’s its specific heat? J/g o C 0.03 J/g o C, Mercury Example #2: 100g of an unknown metal cools 60  20 o C by absorbing 132 cal of heat. What metal is it?