What is a mole chemistry notes?
What is a mole chemistry notes?
A mole is defined as the amount of substance containing the same number of discrete entities (atoms, molecules, ions, etc.) The molar mass of an element (or compound) is the mass in grams of 1 mole of that substance, a property expressed in units of grams per mole (g/mol) (see Figure 1).
What is a mole in chemistry GCSE?
Chemists measure the amount of a substance in a unit called ‘the mole’. It allows chemists to make predictions about the masses of different substances that are involved in reactions. One mole is the Avogadro number of particles (atoms, molecules , ions or electrons ) in a substance.
What is the symbol for mole?
symbol mol
The mole, symbol mol, is the SI unit of amount of substance. One mole contains exactly 6.022 140 76 x 1023 elementary entities.
WHAT IS MR in moles?
The molar mass of a substance is the mass of one mole of that substance. It is equal to: the relative atomic mass or A r in grams for atoms and metals. the relative formula mass or M r in grams for molecules and compounds.
What are the revision notes for CIE IGCSE?
CIE IGCSE Chemistry: Revision Notes 1 The Particulate Nature of Matter 1.1 The Particulate Nature of Matter 1.1.1 Kinetic Theory 1.1.2 States of Matter 1.1. 2 Experimental Techniques More
Which is an example of a mole in chemistry?
The mole is the unit representing the amount of atoms, ions, or molecules. One mole is the amount of a substance that contains 6.02 x 1023 particles (Atoms, Molecules or Formulae) of a substance (6.02 x 10 23 is known as the Avogadro Number).
Which is part of the CIE IGCSE Chemistry Syllabus?
Designed for the 0620 / 0971 syllabus. 1. The Particulate Nature of Matter 2. Experimental Techniques 3. Atoms, Elements & Compounds 4. Stoichiometry 5. Electricity & Chemistry 6. Chemical Energetics 7. Chemical Reactions 8. Acids, Bases & Salts
How to calculate the mass of a mole?
CALCULATING MASS Equation: Mass of Substance (grams) = Moles x Mr Example: Substance Amount Mr Mass H2O 0.5 moles 18 ( 0.5 x 18 ) = 9 g NaCl 3 moles 58.5 ( 3 x 58.5 ) = 175.5 g K2CO3 0.2 moles 138 ( 0.2 x 138 ) = 27.6 g (NH4)2SO4 2.5 moles 132 ( 2.5 x 132 ) = 330 g