Homework given 3-6-00
Grams to moles to atoms
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1. Calculate the number of moles in each of the following masses:
a. 0.039 g of palladium
b. 8200 g of iron
c. 0.0073 kg of tantalum
d. 0.00655 g of antimony
e. 5.64 kg of barium
f. 3.37 x 10-6 g of molybdenum
2. Calculate the mass in grams of each of the following amounts:
a. 1.002 moles of chromium
b. 550 moles of aluminum
c. 4.08 x 10-8 moles of neon
d. 7 moles of titanium
e. 0.0086 moles of xenon
f. 3.29 x 104 moles of lithium
3. Calculate the number of atoms in each of the following amounts:
a. 17.0 moles of germanium
b. 0.6144 moles of copper
c. 3.02 moles of tin
d. 2.0 x 106 moles of carbon
e. 0.0019 moles of zirconium
f. 3.227 x 10-10 moles of potassium
4. Calculate the number of moles in each of the following quantities:
a. 6.022 x 1024 atoms of cobalt
b. 1.06 x 1023 atoms of tungsten
c. 3.008 x 1019 atoms of silver
d. 950,000,000 atoms of plutonium
e. 4.61 x 1017 atoms of radon
f. 8 trillion atoms of cerium
5. Calculate the number of atoms in each of the following masses:
a. 0.0082 g of gold
b. 812 g of molybdenum
c. 2.00 x 102 mg of americium
d. 10.09 kg of neon
e. .0705 mg of bismuth
f. 37 g of uranium
6. Calculate the mass of each of the following:
a. 8.22 x 1023 atoms of rubidium
b. 9.96 x 1026 atoms of tellurium
c. 88,300,000,000,000 atoms of radium
d. 2.94 x 1017 atoms of hafnium
7. Calculate the number of moles in each of the following masses:
a. 45.0 g of acetic acid
b. 7.04 g of lead (II) nitrate
c. 5000 kg of iron (III) oxide
d. 12.0 mg of C2H5NH2 (ethylamine)
e. 0.00322 g of stearic acid (C17H35COOH)
f. 50.0 kg of ammonium sulfate
8. Calculate the mass of each of the following amounts:
a. 3.00 moles of selenium oxybromide SeOBr2
b. 488 moles of calcium carbonate
c. 6.00 x 10-8 moles of nicotine C10H14N2
d. 2.50 moles of strontium nitrate
e. 3.50 x 10-6 moles of uranium hexafluoride UF6
9. Calculate the number of molecules in each of the following:
a. 4.27 moles of tungsten (VI) oxide, WO3
b. 0.00300 moles of strontium nitrate
c. 72.5 moles of toluene, C6H4CH3
d. 5.11 x 10-7 moles of vitamin E, C29H50O2
e. 1500 moles of hydrazine, N2H4
f. 0.989 moles of nitrobenzene, C6H5NO2
10. Calculate the number of molecules in each of the following:
a. 285 g of iron (III)phosphate
b. 0.0084 g of C5H5N
c. 85 g of (CH3)2CHCH2OH
d. 4.6 x 10-4 g of mercury (II) acetate
e. 0.0067 g of lithium carbonate
11. Calculate the mass of each of the following:
a. 8.39 x 1023 molecules of F2
b. 6.82 x 1024 molecules of beryllium sulfate
c. 7.004 x 1026 molecules of chloroform, CHCl3
d. 31 billion molecules of chromium (III) formate, Cr(CHO2)3
e. 6.3 x 1018 molecules of nitric acid, HNO3
f. 8.37 x 1025 molecules of freon 114, C2Cl2F4
12. A chemist needs 22.0 g of phenol, C6H5OH for an experiment. How many moles is this?
13. A student needs 0.015 moles of iodine crystals, I2, for an experiment. What mass of iodine crystals should the student obtain?
14. How many moles are in each:
a. 453.6 g of sucrose, table sugar, C12H22O11
b. 453.6 g of table salt
15. What is the mass of aluminum that would have the same number of atoms as 6.35 g of cadmium?
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