Worksheet 2 - 6.00 g. 6. Determine the mass in grams of 2.0...

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Dr. Ramesh Arasasingham WORKSHEET 2 1. What is the average atomic mass of a boron atom in a natural sample of 10,000 boron atoms? Do any of the boron atoms actually have this mass? Explain. 2. Lithium exists as two isotopes: lithium-6 and lithium-7. Given that the average atomic mass of lithium is 6.9 amu, is the ratio of lithium-6 to lithium-7 nearly 10 to 90, 50 to 50, or 90 to 10? Explain. 3. The molar mass of naturally occurring chlorine, which consists of a mixture of 35 Cl (34.9689 amu) and 37 Cl (36.9659 amu), is 35.453 g. What is the natural abundance of each isotope. 4. Determine how many carbon-12 atoms are in a sample that has a mass of 6.00 g. 5. Determine how many moles of atoms are in a sample of natural sodium that has a mass of
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Unformatted text preview: 6.00 g. 6. Determine the mass in grams of 2.0 mols of a sample of natural gold. 7. Determine the mass in grams of a sample of natural copper that has 25 atoms. 8. Which has more atoms: 24.02 g of carbon or 56.18 g of silicon? Explain. 9. Iron is important for the transport of oxygen by red blood cells. If there are about 2.0 x 10 13 red blood cells in the body containing 3.0 g of iron, how many iron atoms are in each red blood cell on the average? 10. Only one isotope of this element occurs in nature. One atom of this isotope has a mass of 9.123 x 10-23 g. Identify the element and give its atomic mass....
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This note was uploaded on 11/19/2010 for the course CHEMISTRY Chem 1A Di taught by Professor Rameshdarasasingham during the Spring '10 term at UC Irvine.

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