4. Let's try another atomic mass problem. Suppose you have a mixture of two chlorine isotopes. The mixture is 40% Chlorine-37 and 60% Chlorine-35. Predict the atomic mass of this mixture. Hint: This is NOT nature's abundance of chlorine. You can check your answer by clicking "My Mixture" under isotope mixture. Next, create the mixture described in the problem. 35.8 amu 36.2 amu 36.0 amu

4. Let's try another atomic mass problem. Suppose you have a mixture of two chlorine isotopes. The mixture is 40% Chlorine-37 and 60% Chlorine-35. Predict the atomic mass of this mixture. Hint: This is NOT nature's abundance of chlorine. You can check your answer by clicking "My Mixture" under isotope mixture. Next, create the mixture described in the problem. 35.8 amu 36.2 amu 36.0 amu

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 43E: The element europium exists in nature as two isotopes: 151Eu has a mass of 150.9196 u and 153Eu has...

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Click 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.
Reference Section 5-2 to find the atomic masses of 12C and 13C, the relative abundance of 12C and 13C in natural carbon, and the average mass (in u) of a carbon atom. If you had a sample of natural carbon containing exactly 10,000 atoms, determine the number of 12C and 13C atoms present. What would be the average mass (in u) and the total mass (in u) of the carbon atoms in this 10,000-atom sample? If you had a sample of natural carbon containing 6.0221 1023 atoms, determine the number of 12C and 13C atoms present What would be the average mass (in u) and the total mass (in u) of this 6.0221 1023 atom sample? Given that 1 g = 6.0221 1023 u, what is the total mass of I mole of natural carbon in units of grams?
Open the Build a Molecule simulation (http://openstaxcollege.org/l/16molbuilding) and select the Larger Molecules tab. Select an appropriate atoms Kit to build a molecule with two carbon and six hydrogen atoms. Drag atoms into the space above the Kit to make a molecule. A name will appear when you have made an actual molecule that exists (even if it is not the one you want). You can use the scissors tool to separate atoms if you would like to change the connections. Click on 3D to see the molecule, and look at both the space-filling and ball-and-stick possibilities. Draw the structural formula of this molecule and state its name. Can you arrange these atoms in any way to make a different compound? 36. Use the Build a Molecule simulation (http://openstaxcollege.org/l/16molbuilding) to repeat Exercise 2.34, but build a molecule with three carbons, seven hydrogens, and one chlorine. Draw the structural formula of this molecule and slate its name. Can you arrange these atoms to make a different molecule? If so, draw its structural formula and state its name. How are the molecules drawn in (a) and (b) the same? How do they differ? What are they called (the type of relationship between these molecules, not their names)?
Open the Build a Molecule simulation (http://openstaxcollege.org/l/16molbuilding) and select the Larger Molecules tab. Select an appropriate atoms Kit to build a molecule with two carbon and six hydrogen atoms. Drag atoms into the space above the Kit to make a molecule. A name will appear when you have made an actual molecule that exists (even if it is not the one you want). You can use the scissors tool to separate atoms if you would like to change the connections. Click on 3D to see the molecule, and look at both the space-filling and ball-and-stick possibilities. Draw the structural formula of this molecule and state its name. Can you arrange these atoms in any way to make a different compound? 35. Use the Build a Molecule simulation (http://openstaxcollege.org/l/16molbuilding) to repeat Exercise 2.34, but build a molecule with two carbons, six hydrogens, and one oxygen. Draw the structural formula of this molecule and state its name. Can you arrange these atoms to make a different molecule? If so, draw its structural formula and state its name. How are the molecules drawn in (a) and (b) the same? How do they differ? What are they called (the type of relationship between these molecules, not their names).
Open the Build a Molecule simulation (http://openstaxcollege.org/l/16molbuilding) and select the Larger Molecules tab. Select an appropriate atoms Kit to build a molecule with two carbon and six hydrogen atoms. Drag atoms into the space above the Kit to make a molecule. A name will appear when you have made an actual molecule that exists (even if it is not the one you want). You can use the scissors tool to separate atoms if you would like to change the connections. Click on 3D to see the molecule, and look at both the space-filling and ball-and-stick possibilities. Draw the structural formula of this molecule and state its name. Can you arrange these atoms in any way to make a different compound?
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.
The element europium exists in nature as two isotopes: 151Eu has a mass of 150.9196 u and 153Eu has a mass of 152.9209 u. The average atomic mass of europium is 151.96 u. Calculate the relative abundance of the two europium isotopes.
The average atomic masses of some elements may vary, depending upon the sources of their ores. Naturally occurring boron consists of two isotopes with accurately known masses ( 10B, 10.0129 amu and 11B, 11.0931 amu). The actual atomic mass of boron can vary from 10.807 to 10.8 19, depending on whether the mineral source is from Turkey or the United States. Calculate the percent abundances leading to the two values of the average atomic masses of boron from these two countries.
In 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?
Solve the given problem using an element that has three naturally occurring isotopes. Click 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.(a) Write the symbols of the isotopes of boron that are shown as naturally occurring in significant amounts.(b) Predict the relative amounts (percentages) of these boron isotopes found in nature. Explain the reasoning behind your choice.(c) 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.(d) 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.(e) Select “Nature’s” mix of isotopes and compare it to your prediction. How well does…
An unmanned space shuttle mission brings samples back to Earth from Mars. Working with samples from mars, you discover that the isotope abundances on Mars are different from on Earth. You are tasked with calculating the average atomic mass (weight) of nitrogen that exists naturally on Mars. You find that the abundance of nitrogen-15 (atomic mass of 15.000 amu) on Mars is 11.639%, and the rest of the nitrogen (abundance = 100% - 11.639%) is nitrogen-14 (atomic mass 14.003 amu). Using that information, what is the average atomic mass (in amu) of nitrogen on Mars? (answer should have 3 decimal places - only input numbers, not "amu")
On a planet in another galaxy, tellurium exists as only two isotopes, Te123 and Te130. The masses and abundances of these isotopes on the planet are 122.90 amu and 15.000% abundance for Te123, and 129.91 amu and 85.000% abundance for Te130. What is the average atomic mass of tellurium on the planet??