Textbook Question
The atomic masses of hydrogen-2 (deuterium), helium-4, and lithium-6 are 2.014102 amu, 4.002602 amu, and 6.0151228 amu, respectively. For each isotope, calculate
(c) the nuclear binding energy per nucleon.
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Ch.21 - Nuclear Chemistry
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 21, Problem 47
How much energy must be supplied to break a single aluminum-27 nucleus into separated protons and neutrons if an aluminum-27 atom has a mass of 26.9815386 amu? How much energy is required for 100.0 g of aluminum-27? (The mass of an electron is given on the inside back cover.)
Verified step by step guidance1
Step 1: First, we need to calculate the mass of the aluminum-27 nucleus. This can be done by subtracting the mass of 13 electrons (since aluminum-27 has 13 electrons) from the total mass of the aluminum-27 atom. The mass of an electron is given, so multiply this by 13 and subtract from the total mass of the atom.
Step 2: Next, we need to calculate the mass of 13 protons and 14 neutrons (since aluminum-27 has 13 protons and 14 neutrons). The mass of a proton is 1.007276 amu and the mass of a neutron is 1.008665 amu. Multiply these by the number of protons and neutrons respectively and add the results together.
Step 3: Now, we need to calculate the mass defect. This is done by subtracting the mass of the aluminum-27 nucleus (calculated in step 1) from the total mass of the protons and neutrons (calculated in step 2).
Step 4: Convert the mass defect from amu to kilograms by multiplying by 1.66053906660 x 10^-27 kg/amu.
Step 5: Finally, calculate the energy required to break the nucleus into separated protons and neutrons using Einstein's equation E=mc^2, where m is the mass defect in kilograms and c is the speed of light in meters per second (3.00 x 10^8 m/s). This will give the energy in joules. To find the energy required for 100.0 g of aluminum-27, multiply the energy for a single nucleus by the number of nuclei in 100.0 g of aluminum-27 (which can be found by dividing 100.0 g by the molar mass of aluminum-27 and then multiplying by Avogadro's number).
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Mass-Energy Equivalence
Mass-energy equivalence, expressed by Einstein's equation E=mc², states that mass can be converted into energy and vice versa. In nuclear reactions, the mass of the nucleus before and after the reaction can differ, and this mass difference (mass defect) is converted into energy. Understanding this principle is crucial for calculating the energy required to break apart a nucleus.
Binding Energy
Binding energy is the energy required to separate a nucleus into its individual protons and neutrons. It is a measure of the stability of the nucleus; higher binding energy indicates a more stable nucleus. The binding energy can be calculated using the mass defect of the nucleus, which is the difference between the mass of the separate nucleons and the mass of the nucleus itself.
Recommended video:
Guided course
02:06
Nuclear Binding Energy
Molar Mass and Avogadro's Number
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole. For aluminum-27, the molar mass is approximately 27 g/mol. Avogadro's number (6.022 x 10²³) allows us to convert between moles and the number of atoms or nuclei. This concept is essential for calculating the total energy required for a given mass of aluminum-27 by determining how many nuclei are present in that mass.
Recommended video:
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02:11Molar Mass Concept
Related Practice
Textbook Question
The atomic masses of nitrogen-14, titanium-48, and xenon-129 are 13.999234 amu, 47.935878 amu, and 128.904779 amu, respectively. For each isotope, calculate (a) the nuclear mass.
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Textbook Question
Potassium-40 decays to argon-40 with a half-life of 1.27 * 109 yr. What is the age of a rock in which the mass ratio of 40Ar to 40K is 4.2?
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