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Thermochemistry: The heat energy of chemical reactions • Enthalpy is the amount of ________ transferred during a reaction. The symbol for the change in enthalpy is ∆H. An endothermic reaction is one that ___________ heat from the surroundings. (___ ∆ H) An endothermic reaction feels ______. Example--an “instant” ice pack • An exothermic process is one that _____________ heat to the surroundings. (___ ∆ H) An exothermic reaction feels _____. Example--burning paper gains + cold loses – hot

Thermochemistry: How to measure heat (Energy) changes calorie (cal) A ____________ is the amount of energy (heat) required to raise the temperature of one gram of water by one degree Celsius. The “calorie” written on food is actually not one calorie in chemistry. It is actually 1 __________ (or ____calories) and is written with a capital C (Calorie) to keep the two separate. A ____________ is the SI unit for measuring the amount of energy or heat transferred in chemistry. Write down this conversion factor: kilocalorie 1000 Joule (J) 1 cal = 4.184 J

McDonalds McChicken

McDonalds McDouble

Crunchy Cheetos

So what do we do with all these Calories? Your body will use these Calories as energy to do everyday activities but what if you don’t use all the calories you consume? Your body will either use the energy or it will store it as fat! So people who eat more food than their body can use exercise as a way of releasing the extra energy. But how much exercise do you really need to do in order to burn off those extra Calories?

Exercise! Running and walking are not the same!! Even though you can run OR walk a mile, there is a difference. According to David Swain, a Ph.D. in exercise physiology, “When you perform a continuous exercise, you burn five Calories for every liter of oxygen you consume and running in general consumes a lot more oxygen than walking.” Running burns approximately 100 Calories per mile. SO WHAT DOES THIS MEAN?

I LOVE FOOD!  But I hate running!  To run off the food previously mentioned, this is approximately how long you would have to RUN! 1 McChicken: 1.38 MILES 1 McDouble: 3.10 MILES 1 bag of Cheetos: 3.30 MILES

Thermochemical Reactions A thermochemical reaction is written as follows: 2S + 3O2  2SO3 + 791.4 kJ This equation represents an ___________ reaction since the heat is a ________. H2 + Br2 + 72.80 kJ  2HBr This equation represents an ___________ reaction since the heat is a __________. exothermic product endothermic reactant

Thermochemistry Problems Problem 1: How much heat will be released when 6.5 moles of sulfur reacts with excess oxygen according to the following equation? Also, tell whether it will be exothermic or endothermic! 2S + 3O2  2SO3 ∆H = -791.4 kJ -791.4 kJ 6.5 mol S _______________ X = -2572 kJ 2 mol S Exothermic ~ ∆H means heat is a product!

Phase Changes & Energy Endothermic: melting, evaporating/boiling & sublimation Exothermic: freezing, condensation, & deposition

“Reaction Profiles” Endothermic Exothermic

Calculations in Thermodynamics In order to calculate how much heat is transferred by a thermochemical reaction the equation we use is q = mc∆T q = the ______ lost or gained in the process m = the _____ of the substance c = the ________ _____ ________ The specific heat of water is 4.186 Joules/gram °C ∆T = Change in temperature heat mass specific heat capacity

Calculations Practice Example 1: How many Joules would it take to raise the temperature of 250 g of ice from -20 °C to -5 °C? (The specific heat of ice is 2.108 Joule/gram °C) q = mc∆T q = 250g (2.108 J/g °C)( 15 °C) q = 7905 Joules = 7.9 kJ

More Practice Example 2: How many calories would it take to raise the temperature of 100 grams of Ethyl Alcohol from 30 °C to 50 °C? (The specific heat of Ethyl alcohol is 0.58 cal/g °C) q = mc∆T q = 100 g (0.58 cal/g °C) (20 °C) q = 1160 cal