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Additional problem set: Atomic theory, structure, and properties 1) Four different isotopes of the element sulfur (S) are found naturally. These isotopes are 32 S, 33 S, 34 S, and 36 S. a) Give the number of atomic number, the number of neutrons, and the number of electrons (assuming that there is no charge on the atom) for each isotope. Isotope Atomic # = # protons # of neutrons (=mass number- #protons) # electrons (= # protons is there is no overall charge) 32 S 16 16 16 33 S 16 17 16 34 S 16 18 16 36 S 16 20 16 b) Given the atomic mass of sulfur (found on your periodic table), which is the most abundant isotope? The atomic mass is 32.065, which is closest in weight to that of the 32 S isotope, indicating that most sulfur consists of this element. c) How many moles of S are in 3.00 g? 3.00 g 32.065 g/mol = 0.0936 mol d) How many atoms of S are in 3.00 g? 0.0936 mol 6.02 x 10 23 atoms/mol = 5.63x10 22 atoms e) Given that the density of sulfur is 2.07 g/cm 3 , what is the volume of 3.00 g of S? 3.00 g 2.07 g/cm 3 = 1.45 cm 3 f) When sulfur is heated in the presence of oxygen, sulfur dioxide forms. If 5.99 g of sulfur dioxide is formed, what weight of oxygen must have reacted? The law of conservation of mass says that the combined weight of reactants (materials before a chemical reaction) is equal to the combined weight of products

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