Using chemistry vocabulary 1. Explain the concept of hot and cold. 2. In your own words explain what would happen to a pot of boiling water placed in the center of the room at the start of the block.

1
Using chemistry vocabulary 1. Explain the
concept of hot and cold.2. In your own words
explain what would happen to a pot of boiling
water placed in the center of the room at the
start of the block.
2
Density of water ONLY!!!1.00g 1.00mL1kx
1,000x
3
Energy is the capacity to do work, supply heat,
or both (Gummy bear file)
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Heat (q) energy flows from warmer objects to
cooler objects, SI unit is J joule
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4.18J 1.00cal
4.18J 1.00cal ( heat to raise 1g water 1oC)
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Law of conservation of energy energy is neither
created nor destroyed
Where does it go?
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Thermochemistrystudy of energy changes that
occur duringchemical reactions and state changes
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Chemical potential energy energy stored in
chemical bonds
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Specific Heat (C) the amount of heat it takes
to raise the temperature of 1g of material 1K
(1oC)?T (Tfinal Tinitial)mmass(g)
qheat(J) ToC
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How much heat is needed to raise the temperature
of 750mL of water from 21oC to 88oC? (Answer in J
and cal)p 508 Water 4.18J/(goC)
11
How much heat is needed to raise the temperature
of 750mL of water from 21oC to 88oC? (Answer in J
and cal)p 508 Water 4.18J/(goC)
12
How much heat is needed to raise the temperature
of 750mL of water from 21oC to 88oC? (Answer in J
and cal)p 508 Water 4.18J/(goC)
13
How much heat is needed to raise the temperature
of 750mL of water from 21oC to 88oC? (Answer in J
and cal)p 508 Water 4.18J/(goC)
14
How much heat is needed to raise the temperature
of 750mL of water from 21oC to 88oC? (Answer in J
and cal)p 508 Water 4.18J/(goC)
15
How much heat is needed to raise the temperature
of 750mL of water from 21oC to 88oC? (Answer in J
and cal)p 508 Water 4.18J/(goC)
16
How much heat is needed to raise the temperature
of 750mL of water from 21oC to 88oC? (Answer in J
and cal)p 508 Water 4.18J/(goC)
17
15kJ are supplied to a 750g iron pan. What will
be the temperature change of the pan?
18
15kJ are supplied to a 750g iron pan. What will
be the temperature change of the pan?
19
15kJ are supplied to a 750g iron pan. What will
be the temperature change of the pan?
20
15kJ are supplied to a 750g iron pan. What will
be the temperature change of the pan?
21
15kJ are supplied to a 750g iron pan. What will
be the temperature change of the pan?
22
15kJ are supplied to a 750g iron pan. What will
be the temperature change of the pan?
23
15kJ are supplied to a 750g iron pan. What will
be the temperature change of the pan?
24
15kJ are supplied to a 750g iron pan. What will
be the temperature change of the pan?
25
System is a part of the universe you focus on.
The surroundings are everything outside the
system (rest of the universe).
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Entropy - Disorder - randomness of a system
Enthalpy (H) the heat content of a
systemexothermic heat exits endothermic
heat enters
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Endothermic
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exothermic
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PuzzleCalorimetry measurement of a heat change
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heat change?H -mC?TmmassCspecific
heat?T(Final Temp- Initial Temp)
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A 375g block of iron is placed in 115g of water
and the temperature of the water changes from
11.5oC to 35.1oC. What is the original
temperature of the iron block? Water
4.186J/gIron 0.46J/g
32
A 375g block of iron is placed in 115g of water
and the temperature of the water changes from
11.5oC to 35.1oC. What is the original
temperature of the iron block? Water
4.186J/gIron 0.46J/g
33
A 375g block of iron is placed in 115g of water
and the temperature of the water changes from
11.5oC to 35.1oC. What is the original
temperature of the iron block? Water
4.186J/gIron 0.46J/g
34
A 375g block of iron is placed in 115g of water
and the temperature of the water changes from
11.5oC to 35.1oC. What is the original
temperature of the iron block? Water
4.186J/gIron 0.46J/g
35
A 375g block of iron is placed in 115g of water
and the temperature of the water changes from
11.5oC to 35.1oC. What is the original
temperature of the iron block? Water
4.186J/gIron 0.46J/g
36
A 375g block of iron is placed in 115g of water
and the temperature of the water changes from
11.5oC to 35.1oC. What is the original
temperature of the iron block? Water
4.186J/gIron 0.46J/g
37
A 375g block of iron is placed in 115g of water
and the temperature of the water changes from
11.5oC to 35.1oC. What is the original
temperature of the iron block? Water
4.186J/gIron 0.46J/g
38
A 375g block of iron is placed in 115g of water
and the temperature of the water changes from
11.5oC to 35.1oC. What is the original
temperature of the iron block? Water
4.186J/gIron 0.46J/g
39
A 375g block of iron is placed in 115g of water
and the temperature of the water changes from
11.5oC to 35.1oC. What is the original
temperature of the iron block? Water
4.186J/gIron 0.46J/g
40
A 375g block of iron is placed in 115g of water
and the temperature of the water changes from
11.5oC to 35.1oC. What is the original
temperature of the iron block? Water
4.186J/gIron 0.46J/g
41
A 375g block of iron is placed in 115g of water
and the temperature of the water changes from
11.5oC to 35.1oC. What is the original
temperature of the iron block? Water
4.186J/gIron 0.46J/g
42
A 375g block of iron is placed in 115g of water
and the temperature of the water changes from
11.5oC to 35.1oC. What is the original
temperature of the iron block? Water
4.186J/gIron 0.46J/g
43
A 375g block of iron is placed in 115g of water
and the temperature of the water changes from
11.5oC to 35.1oC. What is the original
temperature of the iron block? Water
4.186J/gIron 0.46J/g
44
A hot (225oC) 215g block is placed in 179mL of
water at 22oC. The water temperature raises to
49oC (the block cools to 49oC). What is the
specific heat of the block?
45
A hot (225oC) 215g block is placed in 179mL of
water at 22oC. The water temperature raises to
49oC (the block cools to 49oC). What is the
specific heat of the block?
46
A hot (225oC) 215g block is placed in 179mL of
water at 22oC. The water temperature raises to
49oC (the block cools to 49oC). What is the
specific heat of the block?
47
A hot (225oC) 215g block is placed in 179mL of
water at 22oC. The water temperature raises to
49oC (the block cools to 49oC). What is the
specific heat of the block?
48
A hot (225oC) 215g block is placed in 179mL of
water at 22oC. The water temperature raises to
49oC (the block cools to 49oC). What is the
specific heat of the block?
49
A hot (225oC) 215g block is placed in 179mL of
water at 22oC. The water temperature raises to
49oC (the block cools to 49oC). What is the
specific heat of the block?
50
A hot (225oC) 215g block is placed in 179mL of
water at 22oC. The water temperature raises to
49oC (the block cools to 49oC). What is the
specific heat of the block?
51
A hot (225oC) 215g block is placed in 179mL of
water at 22oC. The water temperature raises to
49oC (the block cools to 49oC). What is the
specific heat of the block?
52
a heat term is included in a chemical equation
thermochemical equationCaO H2O Ca(OH)2
65.2kJ (-?H) exothermic the system lost heat
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CaO H2O Ca(OH)2 65.2kJ (-?H) exothermic,
the system lost heatheat is a product released
to its surroundings
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2NaHCO3 129 kJ Na2CO3 H2O CO2 (?H)
Endothermic, the system gained heat heat is a
reactant
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2NaHCO3 129 kJ Na2CO3 H2O CO2

• How much heat is needed to convert 454g of NaHCO3?

56
2NaHCO3 129 kJ Na2CO3 H2O CO2

• How much heat is needed to convert 454g of NaHCO3?

57
2NaHCO3 129 kJ Na2CO3 H2O CO2

• How much heat is needed to convert 454g of NaHCO3?

58
2NaHCO3 129 kJ Na2CO3 H2O CO2

• How much heat is needed to convert 454g of NaHCO3?

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2H2 O2 ? 2H2O 470kJ

• How much heat will be released if 25g of H2 is
  reacted with oxygen?

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2H2 O2 ? 2H2O 470kJ

• How much heat will be released if 25g of H2 is
  reacted with oxygen?

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2NaHCO3 129 kJ Na2CO3 H2O CO2

• How many joules of heat are needed to convert
  750.000g of NaHCO3 ?

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2NaHCO3 129 kJ Na2CO3 H2O CO2

• How many joules heat is needed to convert 750g of
  NaHCO3?
• 575,893J 50pts
• 575.893kJ 45pts
• 1,151kJ or 1,100,000J 40pts
• Tried 25pts
• Nothing 0pts

63
A 575g iron pan is placed on the stove top with
1250mL of water in it at 18oC. How much heat
energy must the stove give off to heat the pan
and water to 99oC in order to cook some Ramen
Noodles?Water 4.186J/goCIron
0.46J/goC(Mmmmm..mmmm Ramen noodles)
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A 575g iron pan is placed on the stove top with
500mL of water in it at 18oC. How much heat
energy must the stove give off to heat the pan
and water to 100oC in order to cook some Ramen
Noodles?Water 4.186oCIron 0.46J/goCwater
?Jiron ?Jtotal ?J or ?kJ
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CaO(s) H2O(l) Ca(OH)2(s) 65.2kJ How much
heat is released if 168g of CaO is reacted with
water?
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• Homework out
• ½ sheet of paper
• Get Safety goggles
• Write your name on your paper.
• Predict the temperature of ice water in Celsius
  and oF. Explain (1-2 sentences) why you made
  your prediction.

67

• Measure the temperature of the ice water mix.
  Record the measurement.
• Predict the temperature of the ice water mix
  after the deicer has been added. Explain (2-3
  sentences)

68

• Record the actual temperature after the deicer
  has been added.
• What do you think happened Explain (2-3
  sentences).

69

• Predict what will happen to the water in the test
  tube (below). Explain (2-3 sentences).
• Add a test tube with a small amount of water to
  your solution. Stir.

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Heat and Changes of StateEnergy is absorbed or
released when matter changes state.
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When ice melts, it absorbs energy from the
surroundings. As melting proceeds, the liquid and
solid water remain at the same temperature until
all of the ice has melted.
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ADDING ENERGYWhen adding energy, 1 of 2 things
happens1.) Temperature Increases OR2.)
Phase Changes.NOT AT THE SAME TIME!!!!!!!!!!!!!!!
!!!!Draw Phases , i.e, Temp vs Energy Graph
below of ice turning to steam and show two
plateaus.
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For (l) (g), an endothermic process, molar
heat of vaporization, D HvapFor water, D Hvap
40.7 kJ
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for (g)? (l) condensation, exothermic molar
heat of condensation.For water D Hcond -40.7 kJ
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How much energy is needed to convert 25g of water
at 100.0oC into 25g of steam at 100.0oC? (state
change)
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How much energy is needed to convert 25g of water
at 23.0oC into 25g of steam at 100.0oC? (state
change)
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Heat of solutiondissolving NaOH in water.H2O
NaOH(s) Na(aq) OH-(aq) D Hsoln
-445.1kJ/mol
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Write a procedure (with data and calculations )
for the creation of 100mL of a 0.125M MgSO4
(MgSO4.7H2O) solution. Create your solution in
a 100mL graduated cylinder and bring it to me.
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Specific Heat capacity (specific heat) the
amount of heat it takes to raise the temperature
of 1g of material 1K(1oC)Water 4.186J/gIron
0.46J/gWhat would heat up faster water or iron?
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After this reaction will the system be cooler?
After the reaction will the reactants be closer
to each other?
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When 250 J of heat is added to15 g of X at 21C,
thetemperature increases to 85C.What is the
specific heat of theX?
85
If the mixture gets colder is the reaction
gaining or releasing heat?2 solutions react and
the temperature of this 125mL mixture (assume
100 water) drops 3.5oC. How much energy was
gained by this reaction?