# Topics 1-5 Review ```A student taught by Ms. Cook:__________________________
Period:________
Unit 6 Review: Topics 1-5
This packet is FOR YOU to learn since you will be taught the material directly FROM ME the
teacher.
There is homework at the end due on Friday 3/29/19 @ the door.
Topics Reviewed:
Topic 1: Specific Heat Capacity
Topic 2: Heating Curves
Topic 3: Heating Curve Calculations
Topic 4: Calorimetry
Topic 5: Solubility & Solubility Curves
Monday
18
Topic 1 & 2 ET
Topic 2 Due
25
Calorimetry Pre Lab
Quiz
Topic 4 Due
Post Spring Break March 2019 – Unit 6 Calendar
Tuesday
Wednesday
Thursday
19
20
21
Topic 3 Due
No School Deer Park
Ms. Cook out for PD.
Fire
No School Deer Park
Fire
26
27
28
Calorimetry Lab
ACT IA3
New Seats!
Dismissal @ 12
Topics 1-5 Review
Topic 5 Due
April 2019 – Unit 6 Calendar
Wednesday
Thursday
3
4
Topic 6 Due
Friday
22
No School Deer Park
Fire
29
Monday
1
Tuesday
2
Ms. Cook Out
Friday
5
HS IA Day
No School
12
8
Ms. Cook out
9
English I EOC – Ms.
Cook Proctoring
10
Topic 7 Due
11
English II EOC
15
Titration Lab
16
Titration Lab
Topic 8 Due
17
Module 6 Review
18
Module 6 Exam
19
No School
22
Ms. Cook on NY Trip
23
Ms. Cook on NY Trip
24
Ms. Cook on NY Trip
25
Ms. Cook on NY Trip
26
Ms. Cook on NY Trip
29
30
1
2
3
A student taught by Ms. Cook:__________________________
Topic 1 Review: Specific Heat
Calculating Specific Heat
Period:________
Q = mc∆T, where Q = heat energy, m = mass, and ∆T = change in temp.
Remember, ∆T = (Tfinal – Tinitial). Show all work and proper units.
1. A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature changes from 25°C to
175°C. Calculate the specific heat capacity of iron.
2. How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22°C to 55°C,
if the specific heat of aluminum is 0.90 J/g°C?
3. A 0.3 g piece of copper is heated and fashioned into a bracelet. The amount of energy transferred by
heat to the copper is 66,300 J. If the specific heat of copper is 390 J/g 0C, what is the change of the
copper's temperature?
Topic 2 Review: Heating Curves
Answer all the questions in complete sentences.
1. Label the phases (solid, liquid, gas) on the curve.
2. Label the phase changes (melting, boiling) on ethanol on the graph.
3. What is the melting point of ethanol? How do you know?
4. What is the boiling point of ethanol? How do you know?
5. In segment AB, explain what is happening to the molecules as heat is being added.
6. In segment BC, explain what is happening to the molecules as heat is being added.
A student taught by Ms. Cook:__________________________
Topic 3: Heating Curve Calculations
Period:________
1. How much heat energy is required to raise the temperature of 15 g of Mercury from 40 °C to 80 °C? The
specific heat capacity of Mercury is 0.671 J/g°C.
a. The heat of vaporization of Mercury is 429 J/mol
b. The heat of fusion of Mercury is 351.4 J/mol
2.
How much heat energy is required to raise the temperature of 30 g of Iron from 1000 °C to 3500 °C? The
specific heat capacity of iron is 0.172 J/g°C.
a. The heat of vaporization of iron is 3070 J/mol
b. The heat of fusion of iron is 1532 J/mol
Topic 4: Calorimetry & Mixture Calorimetry
Q = mc∆T, where Q = heat energy, m = mass, and ∆T = change in temp.
Remember, ∆T = (Tfinal – Tinitial). Show all work and proper units. 1 C = 4184 J
1. How many Calories would be given off by 10.0 g of aluminum when its temperature changes from 22°C to
55°C, if the specific heat of aluminum is 0.90 J/g°C?
2. How many Calories are required to heat 120.0 g of water from 2.0 °C to 24.0 °C? (C of H2O = 4.184 J/g °C)
3. To what temperature will a 50.0 g piece of glass raise if it absorbs 1.26 Calories and its specific heat
capacity is 0.50 J/g°C? The initial temperature of the glass is 20.0°C.
4. Calculate the specific heat of a piece of wood if 1500.0 g of the wood absorbs 16.15 Calories and its
temperature changes from 32°C to 57°C.
(Mixture calorimetry)
5. A piece of metal weighing 59.047 g was heated to 100.0 °C and then put it into 100.0 mL of water (initially
at 23.7 °C). The metal and water were allowed to come to an equilibrium temperature, determined to be
27.8 °C. Assuming no heat lost to the environment, calculate the specific heat of the metal.
A student taught by Ms. Cook:__________________________
Topic 4: Solutions
Solute:
Solvent:
Heterogeneous –
2 types of mixtures
Homogenous –
Homogeneous Vs. Heterogeneous Practice
1. Flat soda pop
2. Cherry vanilla ice cream
4. sugar
5. soil
6. aluminum foil
7. black coffee
8. sugar water
9. city air
10.
paint
11.
alcohol
12.
iron
13.
beach sand
14.
pure air
15.
spaghetti sauce
Period:________
Topic 5: Solubility
1.
Label the following solutions as saturated,
unsaturated, or supersaturated if 40 g of the substance is
a.
KI
b. KNO3
c. NH3
d. NaCl
Describe how to identify saturation:
Saturated:
Unsaturated:
Supersaturated:
2. Label the following solutions as saturated, unsaturated, or supersaturated if 30 g of the substance is
dissolved at 10 °C? Explain your reasoning using evidence from above and the graph.
a. SO2
b. HCl
c. NH4Cl
d. KCl
3. A 100 g sample of water is saturated with NH4Cl at 50 °C. According to reference table G, if the
temperature is dropped to 10 °C how many grams will fall out of solution?
A student taught by Ms. Cook:__________________________
Period:________
Homework!!!! – Due 3/29/19
Topic 1 Specific Heat Calculations
1. Calculate the specific heat capacity of a piece of wood if 1500.0 g of the wood absorbs 67,500 joules of
heat, and its temperature changes from 32°C to 57°C.
2. 100.0 g of 4.0°C water is heated until its temperature is 37°C. Calculate the amount of heat energy needed
to cause this rise in temperature.
3. 25.0 g of mercury is heated from 25°C to 155°C and absorbs 455 joules of heat in the process. Calculate
the specific heat capacity of mercury.
4. What is the specific heat capacity of silver metal if 55.00 g of the metal absorbs 47.3J of heat and the
temperature rises 15.0°C?
Topic 4: Calorimetry & Mixture Calorimetry
1. How many calories are required to raise the temperature of 67.0g of water from 25.7°C to 66.0°C? The
specific heat of H2O is 4.184J/g°C)
2. What is the mass of a sample of metal that is heated from 58.8°C to 88.9°C with a specific heat of
0.4494J/g°C, if Q = 1.08 Calories
3. How many calories are required to raise the temperature of a 10.35g sample of carbon tetrachloride from
32.1°C to 56.4°C? The specific heat of carbon tetrachloride is 0.85651J/g°C.
4. A 5.00 g piece of metal is heated to 100.0oC, then placed in a beaker containing 20.0 g of water at 10.0oC.
The temperature of the water rises to 15.0oC. Calculate the specific heat of the metal.
Topic 2: Heating curves à Homework
1. Label the phases (solid, liquid, gas) on the curve.
2. Label the phase changes (melting, boiling) of the unknown substance on the graph.
3. What is the melting point of the substance? How do you know?
4. What is the boiling point of the substance? How do you know?
5.
Given the chart to the below, identify the substance. Justify your answer.
Sample
Potassium Sulfate
Iron
Silicon Dioxide
Melting Point (°C)
328
1069
1538
1610
Boiling Point (°C)
1749
1689
2861
2230
A student taught by Ms. Cook:__________________________
Topic 3: Heating Curve Calculations à Homework
Period:________
How much heat is required to raise the temperature of 25.0 g of NaCl from 60 °C to 100 °C? The specific heat
capacity of water is 0.786 J/g°C.
a. The heat of vaporization for water: 236 J
b. The heat of fusion for water: 411 J
1. Label the curve with the phases (solid, liquid, gas)
2. Label the curve with the phase changes (melting, boiling)
3. At what temperature does NaCl melt?
4. What temperature does NaCl boil?
5. Draw a dot estimating where the initial temperature for the question is on the graph.
6. Draw a dot estimating where the finial temperature for the question is on the graph.
7. How many equations will you need to use to solve this problem? (Hint: count the numbers of sections
between the initial and final temperatures)
8. Using the information given at the top of the question, solve for the heat required to produce the
temperature change.
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