Chemistry: The Molecular Nature of Matter
7th Edition
ISBN: 9781118516461
Author: Neil D. Jespersen, Alison Hyslop
Publisher: WILEY
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Chapter 0, Problem 12PE
Practice Exercise 0.12
The definition of the size of the atomic mass unit is really quite arbitrary. Could another atom have been chosen, and could the atomic mass unit have been another fraction of the mass of that atom? Give an example. Provide some reasons why scientists would choose
Practice Exercise 0.12
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Naturally occurring silicon consists of three isotopes, 28 Si, 29 Si, and 30 Si, whose atomic masses are 27.9769, 28.9865, and 29.9838, respectively. The most abundant isotope is 28 Si, which accounts for 92.23% of naturally occurring silicon. Given that the observed atomic mass of silicon is 28.0855, calculate the percentages of 29 Si and 30 Si in nature. Please write it on a paper, thank you.
At some point in the future, nuclear chemists have synthesized two stable isotopes of bohrium. Under these conditions, the average atomic mass of bohrium is 270.5294 amu. If bohrium-269 has atomic mass of 269.0129 amu and bohrium 271 has an average mass of 270.9717 amu, what is the percent abundance of bohrium 269? (Express your answer as a percentage to two decimal places).
I am working on question 25 of chapter 2 in the chemistry openstax second edition. The question is what were the percent abundances of two isotopes in if they give two different atomic masses depending on where they are from.
I believe I figured out how to write the math equation for it, but I don't know how to solve the equation.
10.807 = (10.0129*x) + (11.0931 * (1-x))
10.819 = = (10.0129*x) + (11.0931 * (1-x))
I looked up the explanation in the solutions, and my equation looks right, but I have no idea how they solved the algebra portion.
Chapter 0 Solutions
Chemistry: The Molecular Nature of Matter
Ch. 0 - Practice Exercise 0.1
Using the chapter titles...Ch. 0 - Prob. 2PECh. 0 - Prob. 3PECh. 0 - Prob. 4PECh. 0 - Prob. 5PECh. 0 - Prob. 6PECh. 0 - Prob. 7PECh. 0 - Prob. 8PECh. 0 - Prob. 9PECh. 0 - Practice Exercise 0.10 Aluminum atoms have a mass...
Ch. 0 - Practice Exercise 0.11 How much heavier is the...Ch. 0 - Practice Exercise 0.12 The definition of the size...Ch. 0 - Practice Exercise 0.13 Naturally occurring boron...Ch. 0 - Practice Exercise 0.14
Neon, the gas used in neon...Ch. 0 - Prob. 1RQCh. 0 - 0.2 Knowing what we know today, which of the...Ch. 0 - 0.3 In what ways does the atomic theory affect the...Ch. 0 - Shake a few crystals of salt into your hand and...Ch. 0 - Are there any examples of crystals in nature that...Ch. 0 - 0.6 Heat is one form of energy. If a reaction...Ch. 0 - Can you think of a chemical reaction that starts...Ch. 0 - 0.8 Some large biological molecules rely on...Ch. 0 - 0.9 What elements were formed (a) during the first...Ch. 0 - Prob. 10RQCh. 0 - 0.11 What is the predominant element in the solar...Ch. 0 - Prob. 12RQCh. 0 - What physical factors caused elements and minerals...Ch. 0 - Is this separation still occurring on the earth?Ch. 0 - 0.15 What measuring devices did early chemists...Ch. 0 - 0.16 In your own words, describe how Daltons...Ch. 0 - Which of the laws of chemical combination is used...Ch. 0 - Prob. 18RQCh. 0 - Where in an atom is nearly all of its mass...Ch. 0 - What is a nucleon? Which ones have we studied?Ch. 0 - 0.21 How was the charge-to-mass ratio of the...Ch. 0 - 0.22 How did Robert Millikan determine the charge...Ch. 0 - How was the proton discovered?Ch. 0 - What experiment did Rutherford carry out to...Ch. 0 - Why dont we count the electrons when determining...Ch. 0 - Define the terms atomic number and mass number....Ch. 0 - Prob. 27RQCh. 0 - Write the symbols of the isotopes that contain the...Ch. 0 - What is wrong with the following statement? The...Ch. 0 - 0.30 The atomic number of silver, Ag, is 47 and it...Ch. 0 - A certain element X forms a compound with oxygen...Ch. 0 - Nitrogen reacts with a metal to form a compound in...Ch. 0 - Give the numbers of neutrons, protons, and...Ch. 0 - 0.34 Give the numbers of electrons, protons, and...Ch. 0 - Iodine-131 is used to treat overactive thyroids;...Ch. 0 - Prob. 36RQCh. 0 - 0.37 One chemical substance in natural gas is a...Ch. 0 - 0.38 Carbon tetrachloride contains one carbon and...Ch. 0 - If an atom of carbon-12 had been assigned a...Ch. 0 - 0.40 One atom of has a mass that is 9.0754 times...Ch. 0 - Naturally occurring copper is composed of 69.17%...Ch. 0 - Naturally occurring magnesium (one of the elements...Ch. 0 - N2O is often called nitrous oxide or laughing gas,...Ch. 0 - An element has 24 protons in its nucleus. (a)...Ch. 0 - Iron is composed of four isotopes with the...Ch. 0 - 0.46 What color are the protons, neutrons, and...Ch. 0 - 0.47 Immediately after the big bang, helium and...Ch. 0 - Prob. 48RQCh. 0 - Scientists often validate measurements, such as...Ch. 0 - Sir James Chadwick, discovered the neutron. The...
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Average atomic masses listed by JUPAC are based on a study of experimental results. Bromine has two isotopes 79Br and 81Br, whose masses (78.9 183 and 80.9 163 amu) and abundances (50.69% and 49.3 1%) were determined in earlier experiments. Calculate the average atomic mass of bromine based on these experiments.arrow_forwardArgon has three naturally occurring isotopes: 0.3336% 36Ar, 0.063% 38Ar, and 99.60% 40Ar. Estimate the average atomic mass of argon. If the masses of the isotopes are 35.968 u, 37.963 u, and 39.962 u, respectively, calculate the average atomic mass of natural argon.arrow_forwardGather any two of the following items, measure their dimensions, and calculate the number of atoms present in the item. a. a copper penny (pre-1983), density of copper = 8.96g/cm3 b. a nickel (assume that the nickel is pure nickel, Ni), density of nickel = 8.90g/cm3 c. a graphite pencil lead (pure carbon), density of carbon = 2.62g/cm3 d. a helium balloon (assume that the balloon is approximately spherical; the volume of a sphere is V=(43)r3, where r is the radius), density of helium gas = 0.0899 g/Larrow_forward
- Chlorine has two prominent isotopes,37Cl and35Cl . Which is more abundant? How do you know?arrow_forwardWhen we refer to doughnuts or cookies, we often refer to 1doz of them, which corresponds to 12. Why is the dozen an inconvenient number when referring to atoms? Why is Avogadros number, 6.0221023, more convenient?arrow_forwardClick on the site (http://openstaxcollege.org/l/16PhetAtomMass) and select the Mix Isotopes tab, hide the Percent Composition and Average Atomic Mass boxes, and then select the element boron. Write the symbols of the isotopes of boron that are shown as naturally occurring in significant amounts. Predict the relative amounts (percentages) of these boron isotopes found in nature. Explain the reasoning behind your choice. Add isotopes to the black box to make a mixture that matches your prediction in (b). You may drag isotopes from their bins or click on More and then move the sliders to the appropriate amounts. Reveal the Percent Composition and Average Atomic Mass boxes. How well does your mixture match with your prediction? If necessary, adjust the isotope amounts to match your prediction. Select Nature’s mix of isotopes and compare it to your prediction. How well does your prediction compare with the naturally occurring mixture? Explain. If necessary, adjust your amounts to make them match Nature’s amounts as closely as possible. 21. Repeat Exercise 2.20 using an element that has three naturally occurring isotopes.arrow_forward
- Bromine has two stable isotopes: 79Br and 81Br with masses of 78.9183371 amu and 80.9162906 amu. If the average atomic mass for Bromine on Earth is 79.904 amu, what is the mass of 79Br in a 10.0 g sample? Hint: Set the abundance of the 79Br isotope equal to x. Then the abundance of the other isotope will equal 1−x. Your answer should have three significant figures, so round to the nearest hundredth.arrow_forwardIndium has two naturally occurring isotopes: 113In, with an atomic weight of 112.904 amu; and 115In, with an atomic weight of 114.904 amu. If the average atomic weight for In is 114.818 amu, calculate the fraction-of-occurrences of these two isotopes.arrow_forwardChemists generally use the term atomic weight rather than average atomic mass. We state in the text that the latter term is more correct. By considering the units of weight and mass, can you explain why this is so? The response has to be a narrative, in the form of a paragraph showing work (mathematics) wherever applicable. This paragraph should be at least 10 complete sentences. These sentences must be explaining your answer. please type the answerarrow_forward
- A particular element has 2 stable isotopes. If the first isotope has a mass of 14.754 amu and an abundance of 73.54 % and the second isotope has a mass of 15.362 amu, what is the atomic weight of this element. Express your answer to the correct number of significant figures, and include units with your answer.arrow_forwardThere are only two naturally-occuring stable isotopes of boron. The mass and natural abundance of one of them is listed in the table below. Use whatever data you need from the ALEKS Periodic Table to determine the identity, mass and natural abundance of the other isotope, and complete the table. Round your entry for mass to 3 significant digits and your entry for natural abundance to 3 significant digits.arrow_forwardIn 1961, scientists agreed that the atomic mass unit (amu) would be defined as 1/ 12 the mass of an atom of 12C. Before then, it was defined as 1 /16 the average mass of an atom of naturally occurring oxygen (a mixture of 16O, 17O, and 18O). The current atomic mass of oxygen is 15.9994 amu. (a) Did Avogadro’s number change after the definition of an amu changed and, if so, in what direction? (b) Did the definition of the mole change? (c) Did the mass of a mole of a substance change? (d) Before 1961, was Avogadro’s number 6.02x1023 (to three significant figures), as it is today?arrow_forward
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