Introduction to Chemistry: Temperature and Heat Assignment

This chemistry assignment explores the concepts of temperature and heat, focusing on different temperature scales (Fahrenheit, Celsius, Kelvin) and their conversions. The assignment utilizes models to illustrate these concepts, providing critical thinking questions to assess understanding. It covers temperature conversions using provided equations, including converting between Celsius and Fahrenheit and calculating the boiling point of water in Kelvin. Furthermore, the assignment delves into the relationship between temperature and heat, exploring how energy is required to raise the temperature of water, considering mass and specific heat capacity. The assignment also explores heat calculations using the formula: Heat = mass × Specific Heat Capacity × Temperature Change, and the student is asked to calculate the energy required to raise the temperature of different substances and compare their heat capacities. The student provides detailed answers to each question, showing the calculations and reasoning behind them.

Running Head: Heat 1
Temperature and Heat.
Student’s Name
University Affiliation
Date

Heat 2
TEMPERATURE AND HEAT
CHEMACTIVITY 3C
MODEL 1: THREE THERMOMETERS
The three thermometers below are identical, except for the labeling of the scales.
CRITICAL THINKING QUESTIONS
1. On the Fahrenheit thermometer, how many degrees are there between the freezing
point and the boiling point of water?
Answer
212 – 32 = 180 Fahrenheit degrees
2. On the Celsius thermometer, how many degrees are there between the freezing point
and the boiling point of water?
Answer
100 – 0 = 100 Celsius degrees
3. On the Kelvin thermometer, how many degrees are there between the freezing point
and the boiling point of water?
Answer
373 – 273 = 100 Kelvins
4. Two of the thermometers have degrees that are the same size. Which two?
The Celsius degree thermometer and the kelvins thermometer
5. Which is bigger, one degree Celsius or one degree Fahrenheit? Explain your answer.

Heat 3
Answer
One degree Celsius is bigger. Since 100 subdivisions on the Degree Celsius scale
represents 100 Degree Celsius while 100 subdivisions on Fahrenheit represents 180
Fahrenheit degrees.
i.e.
1 degree Celsius = 1.8 degree Fahrenheit.
MODEL 2: TEMPERATURE CONVERSIONS
The following equations are useful in converting between temperature units.
K = °C + 273.15 °C =
(°F − 32)
1.8
Note that the ° symbol is not used on the unit
K.
CRITICAL THINKING QUESTIONS
6. Is the first conversion equation consistent with your answer to CTQ 4? How so?
Answer
Yes
7. Use the first equation to find the boiling point of water in kelvins. Is your answer
consistent with the figure in Model 1?
Answer
K = °C + 273.15
Boiling point of water in degree Celsius = 100°C
Temperature in kelvin, K = 100 °C + 273.15= 375.15
Yes, the answer is consistent with the figure in model 1
8. Which equation would you use to convert from Fahrenheit to Celsius?
Answer
°C =
(°F − 32)
1.8
9. Water boils at 212 °F. Use the correct equation to convert that into °C. Check your
answer with the figure.
Answer

Heat 4
°C =
(212 − 32)
1.8
°C = 180/1.8
°C =100
10. Room temperature is about 70 °F. What is that in °C?
Answer
°C =
(70− 32)
1.8
°C = 38/1.8
°C =21.11
11. Rearrange the second equation to make a new equation you could use to convert from
°C to °F.
°C =
(°F − 32)
1.8
°F= (°C x 1.8) + 32
12. Check your equation by doing CTQ10 backwards.
Answer
°F= (°C x 1.8) + 32
70= (°C x 1.8) + 32
70 – 32 = °C x 1.8
38= °C x 1.8
38/1.8 = °C
21.11= °C
MODEL 3: CONVERTING TEMPERATURE TO HEAT
In scientific usage, heat and temperature are not the same thing. However, they
can be converted into one another.
Fact: It takes 4.184 J of energy to raise 1 gram of water by 1 °C.
13. How much energy do you think it will take to raise the temperature of2 g of water by
1 °C? Explain your answer.
Answer

Heat 5
Since, there is no change in temperature and the mass of water has doubled from 1g
to 2g then the energy required will be twice.
i.e. Energy = 4.184 x 2 = 8.368 J
14. How much energy do you think it will take to raise the temperature of 1 g of water
from room temperature (about 20 °C) to body temperature (about 37 °C)? Explain
your answer.
Answer
1°C = 4.184 J
20°C=??
H = 20 °C x 4.184J = 83.68 J
1 °C
It takes 4.184 J of energy to raise 1 gram of water by 1 degree Celsius. Since the
mass is constant and the substance is the same (water) then it will require 20 times
more energy to raise the temperature to 20 degrees Celsius.
15. How much energy do you think it will take to raise the temperature of 2 g of water by
2 °C? Explain your answer.
Answer
Step 1
1 g = 4.184 J
2 g =?
2 g x 4.184 J = 8.368 J
1 g
Explanation: Raising 1 g of water by one degree requires 4.184 J, since the mass of
water has doubled the energy will double too, hence 8.368 J
Step 2
8.368 J
2g = 1 °C = 8.368 J
2g = 2 °C =?
H= 2 °C x 8.368 J
1 °C
H= 16.736 J
Explanation: Raising 2 g of water by one degree requires 8.368 J, since the
temperature of water has doubled the energy will double too, hence 16.736 J

Heat 6
16. If you drink 1 cup (about 250 g) of ice water that is initially at 0 °C, how much
energy will your body have to use to warm it up to body temperature?
Answer
Mass = 250g
Temperature change = 37-0= 37 °C
H= 250g x 4.184 J/g °C x 37 °C
H= 38702.0 J
MODEL 4: CONVERTING TEMPERATURE TO HEAT, II
Heat = mass × Specific Heat Capacity × Temperature Change Δ
Substance Specific Heat Capacity (J/g °C)
Water 4.184
Ethanol 2.42
Aluminum 0.903
17. Identify the symbols used for:
a. heat: H
b. mass: m
c. specific heat capacity: c
d. temperature change: Δ T
18. What is the specific heat capacity for water? (Include the units.)
Answer
c= 4.184 J/g °C
19. Use the equation above to calculate the heat required to raise the temperature of 2
g of water by 2 °C. Write all units clearly!
Answer
Heat = 2 g x 4.184 J/g °C x 2 °C
= 16.736 J
20. Did the units cancel to give the units you were hoping to get in your answer?
Answer
Yes, they cancelled to give J, which is the unit for heat quantity.
21. Is your answer to CTQ 19 consistent with your answer to CTQ 15?
Answer
Yes, both gave H= 16.736 J
22. How much energy does it take to raise the temperature of 2 g of aluminum by 2 °C?
Answer

Heat 7
Heat = 2 g x 0.903 J/g °C x 2 °C
= 3.612 J
23. If you added 4 J of heat to 1 g of water and 1 g of aluminum, which would
increase in temperature more? Explain your answer. (Don’t do any
calculations.)
Answer
Aluminum will increase in temperature more.
Explain
Aluminum has a lower specific heat capacity (0.903 J/g °C) than water (4.184 J/g °C) it
therefore requires less energy per unit gram to raise it pee a degree Celsius. Hence, a 4 J
heat will cause a relatively higher temperature in aluminum than water of the same mass.
24. In a complete sentence or two, explain why C is called the “heat capacity.”
Answer
Heat capacity, C, is the amount of heat energy needed to increase temperature of
substance by one degree Celsius.
References
Fischer-Cripps, A. C. (2012). The chemistry companion. Boca Raton, FL: CRC Press.

Heat 8
Goldberg, D. E. (2014). Beginning chemistry. New York: McGraw-Hill Education.
Spellman, F. R., & Whiting, N. E. (2013). Handbook of mathematics and statistics for the
environment. Boca Raton: Taylor & Francis.