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3) Setting up using the conversion factors of molar mass and/or Avogadro's number: a) A modern penny weighs 2.5 g, but contains only 0.63 g of copper(Cu). How many copper atoms are present in a modern penny? See Problem 3.20 b) Determine the number of atoms of sulfur in 5.10 moles of sulfur? See Problem 3.13 4) Which sample has more atoms: 1.10 g of hydrogen atoms, or 14.7 g of chromium atoms? See Problem 3.21 3.3 Molecular Mass 5) Calculate the molecular mass (in amu) and molar mass(in grams) of each of the following substances: See Problem 3.23-24 CH4 a) b) c) K₂SO4 Ca3(PO4)2

3) Setting up using the conversion factors of molar mass and/or Avogadro's number: a) A modern penny weighs 2.5 g, but contains only 0.63 g of copper(Cu). How many copper atoms are present in a modern penny? See Problem 3.20 b) Determine the number of atoms of sulfur in 5.10 moles of sulfur? See Problem 3.13 4) Which sample has more atoms: 1.10 g of hydrogen atoms, or 14.7 g of chromium atoms? See Problem 3.21 3.3 Molecular Mass 5) Calculate the molecular mass (in amu) and molar mass(in grams) of each of the following substances: See Problem 3.23-24 CH4 a) b) c) K₂SO4 Ca3(PO4)2

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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questions 3-5 please

3.1 Atomic Mass 1) Chlorine exists as a mixture of 2 major isotopes, Chlorine-35 and Chlorine-37. Calculate the average atomic mass for Chlorine. See Problem 3.5 Isotope amu Abundance(%) 34.968 35 17 CL 37 17 Cl Fun Sheet to Accompany Chapter 3 → Explain why the atomic masses on the periodic table are decimals. 36.956 3.2 Molar Mass of an Element and Avogadro's Number 2) Setting up using the conversion factor between the number of atoms in a mole & Avogadro's number, convert 6.00 x 10⁹ atoms of Cobalt(Co) to moles of cobalt atom. See Problem 3.14 75.53 3) Setting up using the conversion factors of molar mass and/or Avogadro's number: 24.47 a) A modern penny weighs 2.5 g, but contains only 0.63 g of copper(Cu). How many copper atoms are present in a modern penny? See Problem 3.20 b) b) Determine the number of atoms of sulfur in 5.10 moles of sulfur? See Problem 3.13 c) 4) Which sample has more atoms: 1.10 g of hydrogen atoms, or 14.7 g of chromium atoms? See Problem 3.21 3.3 Molecular Mass 5) Calculate the molecular mass (in amu) and molar mass(in grams) of each of the following substances: See Problem 3.23-24 a) CH4 K₂SO4 Ca3(PO4)2
Transcribed Image Text:3.1 Atomic Mass 1) Chlorine exists as a mixture of 2 major isotopes, Chlorine-35 and Chlorine-37. Calculate the average atomic mass for Chlorine. See Problem 3.5 Isotope amu Abundance(%) 34.968 35 17 CL 37 17 Cl Fun Sheet to Accompany Chapter 3 → Explain why the atomic masses on the periodic table are decimals. 36.956 3.2 Molar Mass of an Element and Avogadro's Number 2) Setting up using the conversion factor between the number of atoms in a mole & Avogadro's number, convert 6.00 x 10⁹ atoms of Cobalt(Co) to moles of cobalt atom. See Problem 3.14 75.53 3) Setting up using the conversion factors of molar mass and/or Avogadro's number: 24.47 a) A modern penny weighs 2.5 g, but contains only 0.63 g of copper(Cu). How many copper atoms are present in a modern penny? See Problem 3.20 b) b) Determine the number of atoms of sulfur in 5.10 moles of sulfur? See Problem 3.13 c) 4) Which sample has more atoms: 1.10 g of hydrogen atoms, or 14.7 g of chromium atoms? See Problem 3.21 3.3 Molecular Mass 5) Calculate the molecular mass (in amu) and molar mass(in grams) of each of the following substances: See Problem 3.23-24 a) CH4 K₂SO4 Ca3(PO4)2
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