Textbook Question
Indicate whether each of the following statements describes potential or kinetic energy:
b. kicking a ball
1
views
Ch.3 Matter and Energy
Timberlake14th EditionChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9781292472249
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch.1 Chemistry in Our Lives19
- Ch.2 Chemistry and Measurements80
- Ch.3 Matter and Energy53
- Ch.4 Atoms and Elements58
- Ch.5 Nuclear Chemistry42
- Ch.6 Ionic and Molecular Compounds57
- Ch.7 Chemical Quantities and Reactions38
- Ch.8 Gases30
- Ch.9 Solutions50
- Ch.10 Acids and Bases and Equilibrium64
- Ch.11 Introduction to Organic Chemistry: Hydrocarbons77
- Ch.12 Alcohols, Thiols, Ethers, Aldehydes, and Ketones82
- Ch.13 Carbohydrates54
- Ch.14 Carboxylic Acids, Esters, Amines, and Amides91
- Ch.15 Lipids61
- Ch.16 Amino Acids, Proteins, and Enzymes84
- Ch.17 Nucleic Acids and Protein Synthesis86
- Ch.18 Metabolic Pathways and ATP Production73
Timberlake14th EditionChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9781292472249Not the one you use?Change textbook
Chapter 3, Problem 29
If the same amount of heat is supplied to samples of 10.0 g each of aluminum, iron, and copper all at 15.0 °C, which sample would reach the highest temperature (see TABLE 3.11)?
Verified step by step guidance1
Step 1: Understand the relationship between specific heat capacity and temperature change. The specific heat capacity (c) of a substance determines how much heat (q) is required to change the temperature of a given mass (m) of the substance by a certain amount (ΔT). The formula is q = m * c * ΔT.
Step 2: Recognize that the same amount of heat (q) is supplied to each sample. Since the mass (m) of each sample is the same (10.0 g), the temperature change (ΔT) will depend on the specific heat capacity (c) of each metal. Metals with lower specific heat capacities will experience a greater temperature change for the same amount of heat.
Step 3: Refer to the specific heat capacities of aluminum, iron, and copper from Table 3.11 (not provided in the image). Compare the values of specific heat capacity for these metals. Identify which metal has the lowest specific heat capacity.
Step 4: Use the relationship ΔT = q / (m * c) to confirm that the metal with the lowest specific heat capacity will reach the highest temperature when the same amount of heat is supplied.
Step 5: Conclude that the metal with the lowest specific heat capacity from Table 3.11 will reach the highest temperature. Ensure you understand the concept that lower specific heat capacity means less heat is required to increase the temperature of the substance.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
1mWas this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Specific Heat Capacity
Specific heat capacity is the amount of heat required to raise the temperature of one gram of a substance by one degree Celsius. It is a crucial property that varies among different materials, influencing how quickly they heat up or cool down when subjected to the same amount of heat. Metals with lower specific heat capacities will experience a greater temperature increase when the same amount of heat is applied.
Recommended video:
Guided course
02:19
Heat Capacity
Heat Transfer
Heat transfer refers to the movement of thermal energy from one object or substance to another due to a temperature difference. In this context, when equal heat is supplied to different metals, the rate at which each metal's temperature increases depends on its specific heat capacity. Understanding heat transfer is essential for predicting how different materials respond to thermal energy.
Recommended video:
Guided course
02:19Heat Capacity
Thermal Equilibrium
Thermal equilibrium is the state reached when two objects at different temperatures come into contact and exchange heat until they reach the same temperature. In the scenario presented, once heat is supplied to the aluminum, iron, and copper samples, they will eventually reach thermal equilibrium, but the rate at which they do so will depend on their specific heat capacities, affecting which sample reaches the highest temperature first.
Recommended video:
Guided course
02:13Thermal Equilibrium (Simplified) Concept 1
Related Practice
Textbook Question
Use the heat equation to calculate the energy, in joules and calories, for each of the following (see TABLE 3.11):
c. lost when 15.0 g of ethanol, C2H6O, cools from 60.5 °C to −42.0 °C
1
views
Textbook Question
Discuss the changes in the potential and kinetic energy of a roller-coaster ride as the roller-coaster car descends from the top of the ramp.
Textbook Question
Using the energy values for foods (see Table 3.8), determine each of the following (round off the answer for each food type to the tens place): d. the grams of fat in one avocado that has 410 kcal, 13 g of carbohydrate, and 5 g of protein
1
views
Textbook Question
Using the energy values for foods (see TABLE 3.7), determine each of the following (round off the answer for each food type to the tens place):
a. the total kilojoules in two tablespoons of crunchy peanut butter that contains 6 g of carbohydrate, 16 g of fat, and 7 g of protein
2
views
Textbook Question
Indicate whether each of the following statements describes potential or kinetic energy:
c. the energy in a lump of coal