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Understanding Molar Mass: Calculating the Mass of Compounds

This lesson from March 6, 2012, focuses on the concept of moles and how to calculate molar mass. Students will learn about the mole as a unit for measuring quantities of particles, defined as 6.02 x 10^23. The lesson covers essential concepts such as defining the mole, the significance of carbon-12 in molar mass, and step-by-step instructions for calculating the molar mass of compounds. Homework includes exercises on calculating molar mass, with a reminder that Friday is the last day to submit last week's work.

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Understanding Molar Mass: Calculating the Mass of Compounds

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  1. March 6, 2012 AGENDA: 1 – Bell Ringer & Part. Log 2 – Intro: Weekly Raffle! 3 – Review Homework 4 – CN: The Mole and Molar Mass Today’s Goal: Students will be able to calculate molar mass. Homework • Calculating Molar Mass • Friday is the Last Day to turn in Last Week’s Work

  2. Cornell Notes • Topic: The Mole and Molar Mass • Date: 3/6/2012 • A mole is a quantity used to measure the amount of matter present. • Like a dozen = 12 • A mole = 6.02 x 1023 • A dozen doughnuts = 12 doughnuts • A mole of carbon = 6.02 x 1023 atoms (particles) of C What is the mole and how is it defined?

  3. Cornell Notes (continued) What is molar mass? • Since the mole is always the same number, a mole of different elements or compounds will have different masses. • The mass of 1 mole was defined by Carbon-12. • 1 mole of carbon = 12 g 1 mol • 6.02 x 1023 atoms carbon = 12 g

  4. Cornell Notes (continued) How do you calculate molar mass? • Determine types of atoms in a compound. • Find their atomic masses. • Sum all masses! Units = g / mol

  5. Practice Problems (Left Side) NaCl = Na = Cl = 58.5 g 1 mol Ag = 107.9 g 1 mol LiNO3 = Li = N = 3 x O = 68.9 g 1 mol 23.0 6.9 35.5 14.0 + + (3x16.0)

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