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Unit 4: The Mole Concept. Learning Goal: To understand the relationship between mass, number and type of particles, volume, and concentration for any chemical. Concept 1: Calculating the Molar Mass of a Pure Substance.
Mole Calculation Worksheet. 1) How many moles are in 40.0 grams of water? 2) How many grams are in 3.7 moles of Na2O? 3) How many atoms are in 14 moles of cadmium? 4) How many moles are in 4.3 x 1022 molecules of H3PO4? 5) How many molecules are in 48.0 grams of NaOH? 6) How many grams are in 4.63 x 1024 molecules of CCl4? 1) 2) 3) 4) Solutions.
This unit uses a discovery-based method to introduce the mole concept without relying on students’ strong background. The lessons contain activities with candy that lead students to develop the rules for mole-item, item-mole, mole-mass, and mass-mole “conversions.”
A mole is a quantity of matter that we use for conversion purposes. We can convert from grams to moles, liters to moles (for gases), and atoms or molecules to moles.
Mole Calculation Practice Worksheet. 2) How many grams are in 4.500 moles of Li2O? 3) How many molecules are in 23.0 moles of oxygen? 4) How many moles are in 3.4 x 1023 molecules of H2SO4? 5) How many molecules are in 25.0 grams of NH3? 6) How many grams are in 8.200 x 1022 molecules of N2I6?
What is a Mole? The value of a mole is fixed, it does not change with the substance being discussed, i.e. one mole of iron, one mole of electrons, and one methane molecules both contain 6.022 \times 10^ {23} particles. This number is known as the Avogadro constant and is typically give the symbols L or NA.
The mole is one of the most important concepts in chemistry, as it allows for quantitative calculation of amounts of substances that may take part in chemical reactions. Various formulas are used to calculate the amount of substance (in mol): n = m M, where n = number of mol and M = molar mass (g mol–1) n = L N
