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Regents Chemistry: Dr. Mintz (

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Chapter(4:(Energy((

116

EnergyChemistry 200

Video Lesson 4.1

Objectives• Define energy. • Demonstrate the difference between endothermic

and exothermic reactions in terms of energy. • Describe how heat is transferred.

What is Energy?• Energy is the ability to do work or produce heat

1.)Potential Energy – positional/stored

2.)Kinetic Energy - motion

Three Forms of Energy1.  Chemical2.  Thermal3.  electromagnetic

Chemical Potential Energy

• Energy stored in a substance because of it’scomposition (chemical bonds)

Chemical Reactions & Energy

• Some reactions release energy (i.e. Combustion of propane) o These are called Exothermic reactionso Freezing of water

• Some reactions absorb/require energy (i.e. photosynthesis) o These are called Endothermic Reactionso Boiling of water

Exothermic Reactions

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Potassium Permanganate and Glycerine Endothermic Reactions

Barium hydroxide and Ammonium chloride Heat Transfer

• Heat can only be measured when it is transferredfrom one piece of matter to another. o Calorimeter – tool that measures heat (units Joules)

Calorimeter• Tool used to measure heat transfer

118

Temperature vs.

HeatChemistry 200

Video Lesson 4.2

How are temperature & heat different? How do we convert between Celsius & Kelvin?

Objective:

I. Heat

A.  the transfer of energy from a body of high temp. to a body of low temp.

B. Unit --> calories or joules

II. TemperatureA.  the measure of average K.E. of the particles

in a substance. (how hot or cold it is)

B. Units are in Celsius (°C) or in Kelvin (K)

III. Heat vs. Temperature

How is Heat different than Temperature?

ex: What is the temp. of 1000g ice? ____

1g ice? ____

What would require more energy to be melted,1000g ice or 1g ice?

0 °C

0 °C

III. Kelvin

A. K = °C + 273

ex1: 35°C = ___ K

K = 35°C + 273= 308K

ex2: 225K = ___ °C

°C = K - 273225 - 273 = -48°C

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B. Absolute Zero -273°C or 0 K

1. Freezing point of H2O = 0°C, molecules are still moving slowly(vibrating) & still have K.E.

2. At absolute zero, the molecules have no K.E.NO MOVEMENT AT ALL!!

Specific Heat

Capacity

Chemistry 200 Video Lesson 4.3

How do we calculate energy gained or lost using specific heat capacity?

Objective: I. Specific Heat Capacity (of a substance)

A. amount of heat required to raise 1g of that substance 1°C

B. different substances have different composition, therefore each have a different specific heat

**specific heat of H2O = 4.18J/g�°C or J/g�K**

(REFERENCE TABLE B)

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II. Calculating Heat

To determine heat absorbed or released in a reaction, we use the following formula:

q = mC∆T

q = heat(in Joules)m = mass of the substanceC = specific heat of the substance (if H2O, look to Ref. Table B)∆T = Tempinitial - Tempfinal

(will always be +)

ex1: How many Joules are absorbed when 50.0g of H2O are heated from 30.2°C to 58.6°C ?

**(Identify known & unknown values always!!!Remember UNITS and SIG FIGS!!!!)**

q = ?m = 50.0gCH2O = 4.18J/g�°C (Ref. Table B)

∆T = 58.6°C - 30.2°C = 28.4°C

q = mC∆T

q = (50.0g)(4.18 J )(28.4°C) g�°C

q = 5935.6J

q = 5940 J (SIG FIGS)

ex2: When 25.0g of H2O are cooled from 20.0°C to 10.0°C, what is the number of Joules of heat energy released?


q = ?m = 25.0gCH2O = 4.18J/g�°C (Ref. Table B)∆T = 20.0°C - 10.0°C= 10.0°Cq = mC∆Tq = (25.0g)(4.18 J )(10.0°C)

g�°Cq = 1045J

q = 1050J (SIG FIGS)

Heat of Fusion

Chemistry 200 Video Lesson 4.4

How do we use heat of fusion (HF) to calculate the energy required to melt or freeze a substance?

Objective:

121

Heat of Fusion (melting)

- the amount of heat energy per unit mass needed to convert a solid to liquid (fusion) or released in liquid to a solid (freezing)

q = heat (in Joules)m = mass of substanceHF = heat of fusion = 334J/g Ref. Table B :)

**How come HF only has J/g & specific heat of H2O (4.18J/g�°C) also has °C or K ?**

q = mHF

ex1: How much heat energy is needed to melt 5.76g of

ice at its melting point?**(Identify known & unknown values always!!!

Remember UNITS and SIG FIGS!!!!)**

q = ?

m = 5.76g

HF = 334J/g

q=mHF

q= (5.76g)(334 J ) g

q = 1923.84 J

q = 1920 J (SIG FIGS)

ex2: If 20.0g of a substance are completely melted at its

melting point & 3444J are absorbed, what is the heat of fusion (HF) of this substance?


q = 3444J

m = 20.0g

HF = ?

q=mHF

3444J = 20.0g(HF)

3444J 20.0g

172.2J/g

HF = 172J/g

(Sig Figs)

= HF

HF =

Heat of Vaporization

Video Lesson 4.5

Objectives• Use the heat of vaporization (Hv) to calculate the

energy required to vaporize or condense a substance.

122

Heat of Vaporization• Vaporization

o Phase change – Liquid to vapor (gas)

• Amount of heat needed to convert a liquidinto a gas at constant pressure andtemperature (or condense a gas to liquid)• TABLE ‘s B & T (constants for water)

o q = mHv

Same amount of Heat

Hfw = 334 J/g

Hvw = 2260 J/g

Heat added

Heat taken away Example #1How much heat is required to vaporize 15.0 grams of water at 100.0 0C?

q = mHv

q = (15.0 g)(2260 J/g)

q = 33900 J

Example #2• How much energy is required to vaporize 10.00

grams of water at its boiling point?

q = mHv

q = (10.0 g)(2260 J/g)

q = 22600 J

123

Name_______________________________________

AmazingIceMeltBlocks

ENGAGE

Guiding Question: Which block (A or B) will melt the ice the faster?

Figure1.

EXPLORE

Demonstration/ Phenomenon: Record your observations as a piece of ice is placed onto each block.

Block Observations/Evidence

A

B

Model/EXPLAIN: Make a labeled model of the experimental set-up at the beginning, rightwhen the ice cubes were placed on the blocks.

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Questions/ELABORATE:

1. Which block felt warmer? Label it A. Which block felt colder?

2. Write “ice melted fast” under the proper block in your drawing.

3. Write “ice melted slow” under the proper block in your drawing.

4. In your own words, explain why the ice melted at different rates.

5. Imagine a new version of this experiment with a frying pan and a plastic foodcontainer; predict which will melt the ice cube faster?

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Practice(Packet:(Energy(

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Video&Lesson&1:&Energy&(

Definition& Characteristics/Facts&&&&&&&&&

Examples& Non>examples&&&&&&&&&

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Definition& Characteristics/Facts&&&&&&&&&

Examples& Non>examples&&&&&&&&&

Exothermic&

Endothermic&

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Heat&Transfer&All substances are made up of small particles, which can be atoms or molecules that are

constantly(moving.(The(faster(the(molecules(are(moving,(the(more(energy(they(have.(The(total(energy(of(motion(in(the(particles(of(a(substance(is(called(thermal&energy.&Temperature&is(the(average(amount(of(energy(of(motion(in(each(particle(of(a(substance.(It(is(a(measure(of(how(hot(or(cold(a(substance(is.((( A&thermometer&is(a(thin(glass(tube(with(a(bulb(on(one(end(that(contains(a(liquid,(usually(mercury(or(colored(alcohol.(Thermometers(work(because(liquids(expand(when(they(are(heated(and(contract(when(they(are(cooled.(Temperature(is(measured(in(units(called(degrees.(On(the(Celsius(scale,(the(freezing(point(of(pure(water(is(0°C(and(the(boiling(point(of(pure(water(is(100°C.(On(the(Kelvin(scale,(the(freezing(point(of(pure(water(is(273(K(and(the(boiling(point(is(373(K.((1. The(Latin(word(calor&means(“heat,”(and(meter&comes(from(the(Greek(word(meaning(“to(

measure.”(What(do(you(think(a(calorimeter&does?((((2. Where(have(you(heard(the(word(calorie&before?(What(do(you(think(a(calorie(is?((

((A(calorimeter(is(an(insulated(container(filled(with(a(liquid,(usually(water.(When(a(hot(object(is(placed(in(the(calorimeter,(heat(energy(is(transferred(from(the(object(to(the(water(and(the(water(heats(up.(The( temperature( change(of( the(water( is( recorded(and(by(using( a( simple(math(equation,(the(amount(of(heat(transferred(can(be(calculated.((

(A(piece(of(gold(at(1000C(is(placed(in(a(simple(calorimeter.(The(starting(temperature(of(the(water(is(300C.((

1. Draw(an(arrow(on(the(diagram(to(represent(the(direction(of(heat(flow.((

2. The(temperature(of(the(water(will(increase(or(decrease?((

3. Name(the(3(forms(of(energy(( ________________________________(( _________________________________(( _________________________________((((

((((

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Exothermic&and&endothermic&reactions&Decide(whether(each(of(these(reactions(is(exothermic(or(endothermic:(a) When(two(chemicals(mix(their(temperature(rises:(_______________(

(b) A(solid(burns(brightly(and(releases(heat,(light(and(sound:(_______________(

(c) When(two(chemicals(are(mixed(their(temperature(drops:((_______________(

(d) Two(chemicals(will(only(react(if(you(heat(them(continually:(_______________(

(e) Plants(take(in(light(energy(for(photosynthesis:(_______________(((Multiple&Choice&

1. _____(What(occurs(when(35Zgram(aluminum(cube(at(100oC(is(placed(in(90.(Grams(of(water(at(25OC(in(an(insulated(cup?(

1) Heat(is(transferred(from(the(aluminum(to(the(water(and(the(temperature(of(the(water(decreases.(

2) Heat(is(transferred(from(the(aluminum(to(the(water(and(the(temperature(of(the(water(increases.((

3) Heat(is(transferred(from(the(water(to(the(aluminum(and(the(temperature(of(the(water(decreases.((

4) Heat(is(transferred(from(the(water(to(the(aluminum(and(the(temperature(of(the(water(increases.(((

2. _____(Which(type(of(energy(is(associated(with(the(random(motion(of(particles(in(a(sample(of(gas?(

1) Chemical(energy(2) Electromagnetic(energy(

3) Nuclear(energy(4) Thermal(energy(

(3. _____(Given(the(balanced(equation(representing(a(reaction:((

(( ( 2H2O((l)((+((energy((!(2H2((g)((+((O2((g)((What(occurs(as(a(result(of(this(reaction?(

1) The(reaction(is(exothermic(and(energy(was(absorbed(2) The(reaction(is(exothermic(and(energy(was(release(3) The(reaction(is(endothermic(and(energy(was(absorbed(4) The(reaction(is(endothermic(and(energy(was(released(

(4. _____(Which(unit(is(used(to(express(the(energy(absorbed(or(released(during(a(

chemical(reaction?(1) Kelvin(2) Joule(

3) Volt(4) Torr

(

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(5. _____(Which(phase(change(is(exothermic?(

1) H2O((s)((!(H2O((g)(2) CO2((s)((!((CO2((l)(

3) H2S((g)((!(H2S((l)(4) NH3((l)((!(NH3((g)

6. _____(Which(of(these(processes(is(always(exothermic?((1) evaporation(2) ((insulation(

3) ((combustion(4) (Melting(

7. ____(When(ammonium(chloride(dissolves(in(water(the(temperature(falls.(The(type(of(energy(change(is(described(as?((

1) ((exothermic(2) ((activated(

3) ((endothermic(4) ((a(decomposition(

8. _____(The(chemical(change(when(a(fuel(burns(can(be(described(as?((1) precipitation(2) ((an(exothermic(reaction(

3) ((a(reversible(reaction(4) ((an(endothermic(reaction(

(Video&Lesson&2:&&Heat&vs.&Temperature((Convert&the&following&temperatures&to&Celsius&(°C)&or&Kelvin&(K)&((((((((((((((Multiple&Choice(

1. _____(Which(statement(defines(the(temperature(of(a(sample(of(matter?(1) Temperature(is(the(measure(of(the(total(electromagnetic(energy(of(the(

particles.(2) Temperature(is(the(measure(of(the(total(thermal(energy(of(the(particles.(3) Temperature(is(the(measure(of(the(average(potential(energy(of(the(particles.((4) Temperature(is(the(measure(of(the(average(kinetic(energy(of(the(particles.(

(2. _____(At(which(temperature(would(atoms(of(a(He(g)(sample(have(the(greatest(average(

kinetic(energy?(1) 25°C(2) 37°C(

3) 273(K(4) 298(K

(1. Z200ºC(!(_____K(

(2. 275(K(!(______°C(

(3. Z40ºC(!(______K(

(4. 150ºC(!(______K(

(5. 445(K(!(______°C(

(6. 0(K(!(________°C(

(

(7. 23ºC(!(_______K(

(8. Z100ºC(!(_____K(

(9. Z196ºC(!(_____K(

(10. ((77(K(!(______°C(

(11. (3.2(x(102(K(!(______°C(

(12. ((45(K(!(_________°C(

(

129

Practice(Packet:(Energy((

http://mintzchemistry.weebly.com(

(3. _____(The(average(kinetic(energy(of(water(molecules(increases(when(

1. H2O((s)(changes(to(H2O(l)(at(0°C(2. H2O(l)(changes(to(H2O(s)(at(0°C(3. H2O(l)(at(10°C(changes(to(H2O(l)(at(20°C(4. H2O(l)(at(20°C(changes(to(H2O(l)(at(10°C(

(4. _____(Which(graph(best(shows(the(relationship(between(Kelvin(temperature(and(

average(kinetic(energy?(((((((((((((((((((

5. _____(At(which(temperature(would(the(molecules(of(a(one(gram(sample(of(water(have(the(lowest(average(kinetic(energy?(

1. 5°C(2. (Z100°C(

3. 5(K(4. 100(K

&Video&Lesson&3:&Specific&Heat&Capacity((

1. How(many(Joules(are(absorbed(when(4.0(g(of(H2O(is(heated(from(12°C(to(39°C(?((((((

2. A(sample(of(H2O(at(17°C(has(250(Joules(of(heat(added.((The(temperature(then(rises(to(33°C.((What(is(the(mass(of(the(H2O(sample?((((

130



3. How(many(Joules(of(energy(is(required(to(heat(12g(of(H2O(from(24°C(to(52°C(?(Also(calculate(how(many(kiloJoules?((((((

4. 655(Joules(is(added(to(12.0g(of(H2O(at(16°C.((What(is(the(final(temperature(of(the(H2O(sample?((((((

5. An(unknown(sample(of(metal(has(a(mass(of(24.5g.((The(addition(of(350(Joules(causes(the(metal(sample(to(increase(in(temperature(by(12°C.((Calculate(the(specific(heat(capacity(of(the(unknown(metal.((((((

6. A(12.4g(sample(of(H2O(has(300(Joules(of(heat(energy(removed.((If(the(final(temperature(of(the(H2O(was(12°C,(what(was(the(initial(temperature(of(the(H2O?(

((((((Video&Lesson&4:&&Heat&of&Fusion&(

1. How(much(heat(is(needed(to(melt(35.0(g(of(ice(at(0(ºC?((Express(your(answer(in(kilojoules.((((((

2. Calculate(the(heat(energy(required(in(joules,(to(melt(5.00(x(102(grams(of(ice(at(0.0°C.((((((

131



3. How(many(Joules(of(heat(is(required(to(melt(42g(of(ice(at(0°C(to(H2O(at(the(same(temperature?((((((

4. What(is(the(mass(of(water(that(releases(65,247(J(when(it(freezes?((((((

5. Calculate(the(heat(of(fusion(for(a(substance(that(requires(1253(joules(to(melt(and(has(a(mass(of(19.9(g.((Is(this(substance(water?((Explain.(

(&&&Video&Lesson&5:&Heat&of&Vaporization&(

1. How(much(energy(is(required(to(vaporize(10.00(grams(of(water(at(its(boiling(point?((((

2. The(heat(of(vaporization(of(a(liquid(is(1,340(J/g.(What(is(the(minimum(number(of(Joules(needed(to(change(45.0(grams(of(liquid(vapor(at(the(boiling(point?(

(((

3. What(is(the(total(number(of(kilojoules(required(to(completely(boil(100.00(g(of(water(at(1000C?(

((((

4. At(1(atm(of(pressure,(25.0(g(of(a(compound(at(its(normal(boiling(point(are(converted(to(a(gas(by(the(addition(of(34,400(J.(What(is(the(heat(of(vaporization(for(this(compound?(

((((

5. How(many(joules(of(energy(are(required(to(vaporize(423g(of(water(at(100oC(and(1(atm?(

132



Using&the&Heat&Formulas&

1. A(5.00Zgram(sample(of(water(is(heated(so(that(its(temperature(increases(from(10.0oC(to(15.0oC.(What(is(the(total(amount(of(energy(absorbed(by(the(water?(((((

2. When(20.0(grams(of(a(substance(are(completely(melted(at(its(melting(point,(3444J(are(absorbed.(What(is(the(heat(of(fusion(for(this(substance?(

((((

3. What(would(be(the(temperature(change(if(3.0(gram(of(water(absorbed(15(Joules(of(heat?(

(((((

4. What(is(the(specific(heat(of(silver(if(a(93.9(g(sample(cools(form(215.0(0C(to(196.0(0C(with(the(loss(of(428(J(of(energy?(

(((((

5. What(is(the(number(of(kilojoules(of(heat(needed(to(change(15(g(of(ice(to(water(a(0oC?((((((

6. In(question(5,(is(heat(being(absorbed(or(released?(Is(this(process(endothermic(or(exothermic?(

(((

7. What(is(the(total(number(of(kilojoules(required(to(completely(boil(200.00(g(of(water(at(1000C?(

(((

133



8. If(100.0(J(are(added(to(20.0(g(of(water(at(30.0oC,(what(will(be(the(final(temperature(of(the(water?(

((((

9. At(1(atm(of(pressure,(25.0(g(of(a(compound(at(its(normal(boiling(point(are(converted(to(a(gas(by(the(addition(of(34,400(J.(What(is(the(heat(of(vaporization(for(this(compound?(

((((

10. The(temperature(of(a(sample(of(water(in(the(liquid(phase(is(raised(30.0oC(by(the(addition(of(3762(J.(What(is(the(mass(of(the(water?(

(

134

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