Ch.2 - Atoms, Molecules & Ions
Chapter 2, Problem 117
A copper wire having a mass of 2.196 g was allowed to react with an excess of sulfur. The excess sulfur was then burned, yielding SO2 gas. The mass of the copper sulfide produced was 2.748 g. (c) Calculate the number of copper ions per cubic centimeter if the density of the copper sulfide is 5.6 g/cm3.
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Textbook Question
(a) The unified atomic mass unit (u) is used to represent the extremely small mass of atoms. How many grams are equivalent to 1 u?
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Textbook Question
(b) The mole is a unit used to represent a very large number of atoms. How many atoms are equivalent to 1 mol of atoms?
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Textbook Question
Match the descriptions (a)–(e) with the following terms: atomic weight, atomic mass, mass number, atomic number, molar mass.
(a) The mass of a specific atom such as one atom of 13C
(b) The quantity determined by the number of protons in an element.
(c) The number of grams in 1 mol of an element
(d) The number of protons and neutrons in an element
(e) The weighted average of the isotopic masses of an element's naturally occurring isotopes
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Textbook Question
Naturally occurring boron consists of two isotopes: 10^B (19.9%) with an isotopic mass of 10.0129 and 11^B (80.1%) with an isotopic mass of 11.009 31. What is the atomic weight of boron? Check your answer by looking at a periodic table.
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Textbook Question
Naturally occurring silver consists of two isotopes: 107^Ag (51.84%) with an isotopic mass of 106.9051 and 109^Ag (48.16%) with an isotopic mass of 108.9048. What is the atomic weight of silver? Check your answer in a periodic table.
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Textbook Question
Magnesium has three naturally occurring isotopes: 24Mg (23.985) with 78.99% abundance, 25Mg (24.986) with 10.00% abundance, and a third with 11.01% abundance. Look up the atomic weight of magnesium, and then calculate the mass of the third isotope.
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