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Practice Exercise 0.14
Neon, the gas used in neon lamps, is composed of 90.483% of
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Chemistry: The Molecular Nature of Matter
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Chemistry & Chemical Reactivity
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- 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.arrow_forwardBromine 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_forwardU-238 is naturally the most abundant form of uranium; however, only U-235 can be used as fuel in a nuclear reactor, so uranium for us in the nuclear industry must be enriched in this isotope. If a sample of enriched uranium has 78.72% of U-235 isotope and 21.28% U-238 isotope, what is the average atomic mass of the Uranium sample?arrow_forward
- An element has the following natural abundances and isotopic masses: 2297% abundance with 27.977 amu, 4.6832% abundance with 28.976, and 3.0872% abundance with 29.974 amu. What is the average atomic mass in amu of this element using four significant figures?arrow_forwardA hypothetical element, E, has two stable isotopes. One isotope has a natural abundance of 66.909% and has an atomic mass of 46.477 u. If the atomic weight of E is 47.918 u, what is atomic mass (in units of u) of the second isotopearrow_forwardThe average atomic mass of copper is 63.55 amu. If the only two isotopes of copperhave masses of 62.94 amu and 64.93 amu, what are the percentages of each?(Think algebra)arrow_forward
- Gather 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_forwardIn the following drawing, the green spheres represent atoms of a certain element. The purple spheres represent atoms of another element. If the spheres of different elements touch, they are part of a single unit of a compound. The following chemical change represented by these spheres may violate one of the ideas of Dalton’s atomic theory. Which one?arrow_forwardA fundamental idea of Daltons atomic theory is that atoms of an element can be neither created nor destroyed. We now know that this is not always true. Specifically, it is not true for uranium and lead atoms as they appear in nature. Are the numbers of these atoms increasing or decreasing? Explain.arrow_forward
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