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100% Workshop 9: The Mole The mole is the unit of measurement for an amount in chemistry and physics. It is defined as the amount of sample that contains as many items as there are atoms in 12 grams of carbon-12 (¹²C isotope). The number of items in 1 mole is called the Avogadro's number: NA = 6.022141 x 1023 1/mol Mole in science, just like a dozen in our everyday life, allows us to quickly count or compare large (huge!) quantities of items (microscopic objects). And since mole is just a number - you can have a mole of anything - atoms, molecules, ions, electrons, photons, etc. For any substance, the number of grams in 1 mole is the same as the number of atomic mass units in the molecular weight of the substance. The molar mass (or molar weight) of a chemical substance is defined as the mass in grams of 1 mole of that substance. The units for molar mass are grams per mole - g/mol. 1:1 The mole provides a bridge between the atom and the macroscopic amounts of material that we work with in the laboratory or in the industrial setting. For example, it allows chemists to determine how many grams of each of the reactants are needed to produce a sought number of grams of product. Part 1: Discussion of mole and mass Discuss these questions among your group members: think about water molecules (H₂0) and sugar molecules (C12H22011) and try to predict the answers in the table below. Just predict - do not use calculator. Do these samples have the same... ...mass? ...volume? ...number of moles? 1 gram of each HI 1 mole of each

100% Workshop 9: The Mole The mole is the unit of measurement for an amount in chemistry and physics. It is defined as the amount of sample that contains as many items as there are atoms in 12 grams of carbon-12 (¹²C isotope). The number of items in 1 mole is called the Avogadro's number: NA = 6.022141 x 1023 1/mol Mole in science, just like a dozen in our everyday life, allows us to quickly count or compare large (huge!) quantities of items (microscopic objects). And since mole is just a number - you can have a mole of anything - atoms, molecules, ions, electrons, photons, etc. For any substance, the number of grams in 1 mole is the same as the number of atomic mass units in the molecular weight of the substance. The molar mass (or molar weight) of a chemical substance is defined as the mass in grams of 1 mole of that substance. The units for molar mass are grams per mole - g/mol. 1:1 The mole provides a bridge between the atom and the macroscopic amounts of material that we work with in the laboratory or in the industrial setting. For example, it allows chemists to determine how many grams of each of the reactants are needed to produce a sought number of grams of product. Part 1: Discussion of mole and mass Discuss these questions among your group members: think about water molecules (H₂0) and sugar molecules (C12H22011) and try to predict the answers in the table below. Just predict - do not use calculator. Do these samples have the same... ...mass? ...volume? ...number of moles? 1 gram of each HI 1 mole of each

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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How can we complete part 1 and finding the number of atoms?
Workshop 9: The Mole The mole is the unit of measurement for an amount in chemistry and physics. It is defined as the amount of sample that contains as many items as there are atoms in 12 grams of carbon-12 (¹²C isotope). The number of items in 1 mole is called the Avogadro's number: Nₐ = 6.022141 x 10²³ 1/mol Mole in science, just like a dozen in our everyday life, allows us to quickly count or compare large (huge!) quantities of items (microscopic objects). And since mole is just a number—you can have a mole of anything—atoms, molecules, ions, electrons, photons, etc. For any substance, the number of grams in 1 mole is the same as the number of atomic mass units in the molecular weight of the substance. The molar mass (or molar weight) of a chemical substance is defined as the mass in grams of 1 mole of that substance. The units for molar mass are grams per mole—g/mol. The mole provides a bridge between the atom and the macroscopic amounts of material that we work with in the laboratory or in the industrial setting. For example, it allows chemists to determine how many grams of each of the reactants are needed to produce a sought number of grams of product. Part 1: Discussion of mole and mass Discuss these questions among your group members: think about water molecules (H₂O) and sugar molecules (C₁₂H₂₂O₁₁) and try to predict the answers in the table below. Just predict—do not use a calculator. <table> <tr> <th>Do these samples have the same…</th> <th>1 gram of each</th> <th>1 mole of each</th> </tr> <tr> <td>…mass?</td> <td></td> <td></td> </tr> <tr> <td>…volume?</td> <td></td> <td></td> </tr> <tr> <td>…number of moles?</td> <td></td> <td></td> </tr> </table>
Transcribed Image Text:Workshop 9: The Mole The mole is the unit of measurement for an amount in chemistry and physics. It is defined as the amount of sample that contains as many items as there are atoms in 12 grams of carbon-12 (¹²C isotope). The number of items in 1 mole is called the Avogadro's number: Nₐ = 6.022141 x 10²³ 1/mol Mole in science, just like a dozen in our everyday life, allows us to quickly count or compare large (huge!) quantities of items (microscopic objects). And since mole is just a number—you can have a mole of anything—atoms, molecules, ions, electrons, photons, etc. For any substance, the number of grams in 1 mole is the same as the number of atomic mass units in the molecular weight of the substance. The molar mass (or molar weight) of a chemical substance is defined as the mass in grams of 1 mole of that substance. The units for molar mass are grams per mole—g/mol. The mole provides a bridge between the atom and the macroscopic amounts of material that we work with in the laboratory or in the industrial setting. For example, it allows chemists to determine how many grams of each of the reactants are needed to produce a sought number of grams of product. Part 1: Discussion of mole and mass Discuss these questions among your group members: think about water molecules (H₂O) and sugar molecules (C₁₂H₂₂O₁₁) and try to predict the answers in the table below. Just predict—do not use a calculator. <table> <tr> <th>Do these samples have the same…</th> <th>1 gram of each</th> <th>1 mole of each</th> </tr> <tr> <td>…mass?</td> <td></td> <td></td> </tr> <tr> <td>…volume?</td> <td></td> <td></td> </tr> <tr> <td>…number of moles?</td> <td></td> <td></td> </tr> </table>
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