The atomic masses of the two stable isotopes of boron, boron-10 (19.78 percent) and boron-11 (80.22 percent), are 10.0129 amu and 11.0093 amu, respectively. Calculate the average atomic mass of boron.
The atomic masses of the two stable isotopes of boron, boron-10 (19.78 percent) and boron-11 (80.22 percent), are 10.0129 amu and 11.0093 amu, respectively. Calculate the average atomic mass of boron.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter2: Chemical Compounds
Section2.11: Molar Mass
Problem 2.15CE
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Transcribed Image Text:Exercises:
1. The atomic masses of the two stable isotopes of boron, boron-10 (19.78 percent) and boron-11
(80.22 percent), are 10.0129 amu and 11.0093 amu, respectively. Calculate the average atomic
mass of boron.
2. How many moles of magnesium (Mg) are there in 87.3 g of Mg?
3. Calculate the number of grams of lead (Pb) in 12.4 moles of lead.
4. Calculate the number of atoms in 0.551 g of potassium (K).
5. What is the molecular mass of methanol (CH4O)?
6. Calculate the number of moles of chloroform (CHC1,) in 198 g of chloroform.
7. How many H atoms are in 72.5 g of isopropanol (rubbingalcohol) C3HgO?
8. Calculate the percent composition by mass of each of the elements in sulfuric acid (H2SO4).
9. Determine the empirical formula of a compound having the following percent composition by
mass: K (24.75%); Mn (34.77%); O (40.51%).
10. Calculate the number of grams of Al in 371 g Al,O3.
11. A sample of a compound containing boron (B) and hydrogen (H) contains 6.444 g of B and 1.803
g of H. The molar mass of the compound is about 30 g. What is its molecular formula?
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