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

heat

gains+ cold

loses– hot

Thermochemistry:How to measure heat (Energy) changes

• 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:

calorie (cal)

kilocalorie

Joule (J)

1 cal = 4.184 J

1000

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 __________.

exothermicproduct

endothermicreactant

Calculating Enthalpy (∆H)• There are two ways to calculate enthalpy.

• Enthalpy can be calculated by the heat of formation of the products minus the reactants using the equation:

• Enthalpy can also be calculated by the energy required to break bonds verses the energy give off when bonds form.

∆H = H (products) – H (reactants)

∆H = Energy of bonds broken – Energy of bonds formed

• Calculate the heat given off by the reaction shown below:

2 B5H9(g) + 12O2(g) 5B2O3(g) + 9H2O(g)

• Heat of Formation

B5H9(g) = 73.2 kJ/mol

B2O3(g) = -1272.77 kJ/mol

O2(g) = 0 kJ/mol

H2O(g) = -241.82kJ/mol

Calculating Enthalpy (∆H)

∆H = H (products) – H (reactants)

[(5 mol B2O3 x -1272.77kJ/mol) +

[(2 molB5H9 x 73.2kJ/mol) + (12 mol O2 x 0kJ/mol)]

(9 mol H2O x -241.82kJ/mol)] – ∆H =

∆H = [-8540.23kJ] - [146.4kJ] = -8686.63kJ

• Find the ∆ H for the following reaction given the following bond energies:

2H2 + O2 2H2O

Bond Energy

H-H 436 kJ/mol

O=O 499 kJ/mol

O-H 463 kJ/mol

Calculating Enthalpy (∆H)

Now we can substitute the values given into the equation:∆H = Energy of bonds broken – Energy of bonds formed

We have to figure out which bonds are broken and which bonds are formed.

2 H-H bonds are broken

∆H = = -481 kJ[(2 x 436) + (1 x 499)] – [4 x 463]

1 O=O bond is broken4 O-H bonds are formed (2 O-H bonds are formed per water molecule, and there are 2 water molecules formed)

Thermochemistry Problems using Stoichiometry

• 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

6.5 mol S X _______________

2 mol S

-791.4 kJ= -2572 kJ

-∆H means heat is a product!

Exothermic ~

Phase Changes & Energy

Endothermic: melting, evaporating/boiling & sublimation

Exothermic: freezing, condensation, & deposition

Endothermic

Exothermic

“Reaction Profiles”

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 = ________ Temp. – ________Temp.

heat

massSpecific heat capacity

InitialFinal

Specific Heat• Specific heat or “c” has units of Joule/gram °C. This refers to the energy needed to change one

gram of the substance one degree Celsius.

Check your understanding:• Which has a higher specific heat? Aluminum or water?

• Why does a pizza roll that you can pickup with your fingers still have the possibility of burning your tongue?

Aluminum. Less heat is required to change aluminum’s temperature.

The pizza sauce inside contains water with a high specific heat.

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

q = 250g (2.108 J/g °C)( 15 °C)

q = 7905 Joules = 7.9 kJ

(2.108 J/g °C) ( -5 °C – (-20 °C))

More Practice

• Example 2: What is the specific heat of Ethyl Alcohol if 100 grams of Ethyl Alcohol was heated from 30 °C to 50 °C when 1160 calories of heat was applied? The specific heat of Ethyl alcohol is 0.58 cal/g °C)

q = mc∆T1160 cal = 100g1160 cal = c x (2000 g °C)c = 0.58 cal/g °C

c ( 50 °C - 30 °C)

Calorimeters•Calorimeters measure heat flow. It measures changes in water temperature after a reaction is performed.

(Constant Pressure)

Bomb CalorimeterUsually studies combustion (Constant Volume)

• Molar heat of fusion (∆Hfus) : the amount of energy required to take 1 mole of a solid to the liquid state.

Example: H2O(s) H2O(l) ∆Hfus = 6.01 kJ

-Heat of fusion is usually greater for ionic solids than molecular solids since ionic solids are more strongly held together.

For ice to water … ∆Hfus= 6.01 kJ/mol

• Molar heat of vaporization (∆H vap): the amount of energy required to take 1 mole of a liquid to the gaseous state.

Example: H2O(l) H2O(g) ∆Hvap = 40.67 kJ

For water to steam … ∆Hvap= 40.67 kJ/mol

Heat of Fusion & Heat of Vaporization

These values are mainly used as conversion factors!

Heating Curve of Water

Calculations Practice1) How much energy is required to raise 75 grams of water from

--20 °C to 20 °C? (∆Hfus= 6.01 kJ/mol and ∆Hvap= 40.67 kJ/mol The specific heat of ice is 2.108 Joule/gram °C, and the specific heat of water is 4.186 joule/gram °C )

q = mc∆T

q = 75g = 3162 Joules = 3.2 kJx (2.108 J/g °C) x (0°C – -20°C)

q = mc∆Tq = 75g = 6279 Joules = 6.3 kJx (4.186 J/g °C) x (20°C –0°C)

Big picture: Solid water heats up, melts, and then liquid water heats up.

75 g H2O X _______________

18.02 g H2O

1 mol H2O = 25.0 kJX _______________

1 mol H2O

6.01 kJ

Energy required = 3.2 kJ + 25.0 kJ + 6.3 kJ = 34.5 kJ