Textbook Question
Consider the data about gold metal in Exercise 5.24(b). c. What is the molar heat capacity of Au(s)?
2
views
Ch.5 - Thermochemistry
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 5, Problem 53b
The specific heat of ethanol, C2H5OH(l), is 2.44 J•g/K. b. Which will require more heat, increasing the temperature of 1 mol of C2H5OH(𝑙) by a certain amount or increasing the temperature of 1 mol of H2O(𝑙) by the same amount?
Verified step by step guidance1
Identify the specific heat capacity of both substances: Ethanol (C_2H_5OH) has a specific heat capacity of 2.44 J/g·K, and water (H_2O) has a specific heat capacity of 4.18 J/g·K.
Calculate the molar mass of ethanol (C_2H_5OH) by adding the atomic masses of its constituent atoms: 2 carbon atoms, 6 hydrogen atoms, and 1 oxygen atom.
Calculate the molar mass of water (H_2O) by adding the atomic masses of its constituent atoms: 2 hydrogen atoms and 1 oxygen atom.
Determine the mass of 1 mole of each substance using their respective molar masses.
Use the formula q = m × c × ΔT to compare the heat required for each substance, where q is the heat absorbed, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
2mWas 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 (or one Kelvin). It is a crucial property that varies between different substances, influencing how much heat is needed to change their temperature. In this question, the specific heat of ethanol is given, which allows for comparison with water's specific heat to determine which substance requires more heat for the same temperature change.
Recommended video:
Guided course
02:19
Heat Capacity
Molar Mass and Moles
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole. Understanding moles is essential in chemistry as it allows for the conversion between mass and the number of particles. In this question, both ethanol and water are considered in terms of moles, which helps in calculating the total heat required to raise their temperatures based on their specific heat capacities.
Recommended video:
Guided course
02:11Molar Mass Concept
Heat Transfer Equation
The heat transfer equation, often expressed as q = mcΔT, relates the heat absorbed or released (q) to the mass (m), specific heat capacity (c), and the change in temperature (ΔT). This equation is fundamental for solving problems involving temperature changes in substances. In this context, it will be used to compare the heat required for both ethanol and water when their temperatures are increased by the same amount.
Recommended video:
Guided course
02:19Heat Capacity
Related Practice
Textbook Question
When a 5.10-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter (Figure 5.18), the temperature rises from 20.5 to 33.2 °C. a. Calculate the quantity of heat (in kJ) released in the reaction.
3
views
Textbook Question
(d) How many kJ of heat are needed to raise the temperature of 10.00 kg of liquid water from 24.6 to 46.2 °C?
2
views
Textbook Question
Consider the data about gold metal in Exercise 5.24(b). b. Suppose that the same amount of heat is added to two 10.0-g blocks of metal, both initially at the same temperature. One block is gold metal, and the other is iron metal. Which block will have the greater rise in temperature after addition of the heat?
2
views
Textbook Question
Two solid objects, A and B, are placed in boiling water and allowed to come to the temperature of the water. Each is then lifted out and placed in separate beakers containing 1000 g of water at 10.0 °C. Object A increases the water temperature by 3.50 °C; B increases the water temperature by 2.60 °C. (a) Which object has the larger heat capacity?
1585
views
1
rank
Textbook Question
(b) Calculate the energy needed for this temperature change.
1316
views