Domanda del libro di testo
What is the mass in grams of each of the following samples?
(a) 1.505 mol of Ti
(b) 0.337 mol of Na
(c) 2.583 mol of U
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Ch.2 - Atoms, Molecules & Ions
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Capitolo 2, Problema 121
A sample of naturally occurring silicon consists of 28^Si (27.9769), 29^Si (28.9765), and 30^Si (29.9738). If the atomic weight of silicon is 28.0855 and the natural abundance of 29^Si is 4.68%, what are the natural abundances of 28^Si and 30^Si?
Guida verificata passo dopo passo1
Identify the given values: atomic weight of silicon (28.0855), natural abundance of 29^Si (4.68%), and the atomic masses of 28^Si (27.9769), 29^Si (28.9765), and 30^Si (29.9738).
Let the natural abundance of 28^Si be x and the natural abundance of 30^Si be y. Since the total natural abundance must sum to 100%, set up the equation x + 4.68% + y = 100%.
Use the average atomic mass formula for silicon, which is the sum of the products of each isotope's mass and its abundance: (27.9769 \(\times\) x) + (28.9765 \(\times\) 4.68\%) + (29.9738 \(\times\) y) = 28.0855.
Solve the system of equations from steps 2 and 3 to find the values of x and y. This involves substituting the value of y from the first equation into the second equation and solving for x.
Once x is found, substitute it back into the equation from step 2 to find y, completing the determination of the natural abundances of 28^Si and 30^Si.
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Atomic Weight and Isotopes
Atomic weight is the weighted average mass of an element's isotopes based on their natural abundances. Isotopes are variants of an element that have the same number of protons but different numbers of neutrons, resulting in different atomic masses. Understanding how to calculate the atomic weight using the masses and abundances of isotopes is crucial for solving problems related to elemental composition.
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04:36
Isotopes
Natural Abundance
Natural abundance refers to the relative proportion of each isotope of an element found in nature. It is usually expressed as a percentage and is essential for calculating the average atomic weight of an element. In this problem, knowing the natural abundance of one isotope allows for the calculation of the abundances of the other isotopes by using the total atomic weight.
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01:26Nature of Energy
Weighted Average Calculation
The weighted average calculation involves multiplying each value by its corresponding weight (or abundance) and then summing these products. This method is used to find the average atomic weight of an element based on its isotopes. In this context, the equation must be set up to include the known abundance of one isotope and solve for the unknown abundances of the others, ensuring that the total adds up to 100%.
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02:42Average Rate Calculation Example
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Magnesium has three naturally occurring isotopes: 24Mg (23.985) with 78.99% abundance, 25Mg (24.986) with 10.00% abundance, and a third with 11.01% abundance. Look up the atomic weight of magnesium, and then calculate the mass of the third isotope.
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Domanda del libro di testo
Copper metal has two naturally occurring isotopes: copper-63 (69.15%; isotopic mass = 62.93) and copper-65 (30.85%; isotopic mass 64.93). Calculate the atomic weight of copper, and check your answer in the periodic table.
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2074
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Domanda del libro di testo
Naturally occurring silver consists of two isotopes: 107^Ag (51.84%) with an isotopic mass of 106.9051 and 109^Ag (48.16%) with an isotopic mass of 108.9048. What is the atomic weight of silver? Check your answer in a periodic table.
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Domanda del libro di testo
Naturally occurring boron consists of two isotopes: 10^B (19.9%) with an isotopic mass of 10.0129 and 11^B (80.1%) with an isotopic mass of 11.009 31. What is the atomic weight of boron? Check your answer by looking at a periodic table.
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