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Chemistry Chapter 10

This chapter explores the fundamental concept of the mole in chemistry, defining it as the amount of substance containing 6.02 × 10²³ representative particles, known as Avogadro's number. It covers methods to quantify substances—by count, mass, and volume—and explains relationships between atomic mass, molar mass, and their significance in calculations. The chapter also details how to determine the mass of a mole of elements and compounds, providing examples for clarity. Mastery of these concepts is critical for solving chemistry problems.

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Chemistry Chapter 10

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  1. Chemistry Chapter 10

  2. You often measure the amount of something by one of three different methods—by count, by mass, and by volume.

  3. What Is a Mole?

  4. mole (mol) • the amount of a substance that contains 6.02 × 1023 representative particles of that substance

  5. Avogadro’s number • the number of representative particles contained in one mole of a substance; equal to 6.02 × 1023 particles

  6. representative particle • the smallest unit into which a substance can be broken down without a change in composition, usually atoms, molecules, or ions

  7. A mole of any substance contains Avogadro’s number of representative particles, or 6.02 × 1023 representative particles.

  8. Converting Moles to Number of Particles

  9. To do this, you must know how many atoms are in a representative particle of the compound. This number is determined from the chemical formula.

  10. To find the number of atoms in a mole of a compound, you must first determine the number of representative particles.

  11. The Mass of a Mole of an Element

  12. Remember that the atomic mass of an element (the mass of a single atom) is expressed in atomic mass units (amu). The atomic masses are relative values based on the mass of the most common isotope of carbon (carbon-12).

  13. The atomic mass of an element expressed in grams is the mass of a mole of the element

  14. molar mass • a term used to refer to the mass of a mole of any substance

  15. The Mass of a Mole of a Compound

  16. You can calculate the mass of a molecule of SO3 by adding the atomic masses of the atoms making up the molecule.

  17. The molar mass (g/mol) of any compound is the mass in grams of 1 mol of that compound. Thus 1 mol of SO3 has a mass of 80.1 g. This is the mass of 6.02 × 1023 molecules of SO3.

  18. To calculate the molar mass of a compound, find the number of grams of each element in one mole of the compound. Then add the masses of the elements in the compound

  19. (9) Key Concept What are three ways to measure the amount of something?Hint • (10) Key Concept Describe the relationship between Avogadro’s number and one mole of any substance.Hint

  20. (11) Key Concept How is the atomic mass of an element related to the molar mass of the element?Hint • (12) Key Concept How can you calculate the mass of a mole of a compound?Hint • (13)How many moles is 1.50 × 1023 molecules NH3?

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