HW 10-20-08

HW 10-20-08 - Calculate the average atomic mass of argon to...

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Joseph Leonard Green P87 #17-20 10/20/08 17. What is the mass in grams of each of the following? a. 1.00 mol Li d. 1.00 molar mass Fe b. 1.00 mol Al e. 6.022 x 10^23 atoms C c. 1.00 molar mass Ca f. 6.022 x 10^23 atoms Ag a. 6.94 g Li d. 55.85 g Fe b. 26.98 g Al e. 12.01 g C c. 40.08 g Ca f. 107.87 g Ag 18. How many moles of atoms are there in each of the following? a. 6.022 x 10^23 atoms Ne c. 3.25 x 10^5 g Pb b. 3.011 x 10^23 atoms Mg d. 4.50 x 10^-12 g O a. 1.00 mol Ne c. 1.57 x 10^3 mol Pb b. 0.50 mol Mg d. 2.8 x 10^-13 mol O 19. Three isotopes of argon occur in nature – Ar-36, Ar-38, and Ar-40.
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Unformatted text preview: Calculate the average atomic mass of argon to two decimal places, given the following relative atomic masses and abundances of each of the isotopes: argon-36 (35.97 amu; 0.337%), argon-38 (37.96 amu; 0.063%), and argon-40 (39.96 amu; 99.600%). 39.95 amu 20. Naturally occurring boron is 80.20% boron-11 (atomic mass =11.01 amu) and 19.80% of some other isotopic form of boron. What must the atomic mass of this second isotope be in order to account for the 10.81 amu average atomic mass of boron? 10 amu (See attached for all work)...
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This note was uploaded on 12/09/2009 for the course CHEM 204 taught by Professor Donnegan during the Spring '08 term at Alabama.

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