'Moles mass' diaporamas de présentation

THE MOLE 1.1.4

405 views • 40 slides

Moles

Moles. Moles EQ: What is a mole? How do Scientist use the mole unit to count?. GPS: SC2 Students will relate how the Law of Conservation of Matter is used to determine chemical composition in compounds and chemical reactions.

830 views • 29 slides

391 views • 27 slides

Chem 1215 Workshop Series Mastering the Basics of Chemistry

Chem 1215 Workshop Series Mastering the Basics of Chemistry. Stoichiometry. Dr. Courtney Dodd. Stoichiometry. The relationships among the quantities of reactants and products involved in chemical reactions. 3CaCl 2 (aq) + 2H 3 PO 4 (aq) ? 6HCl(aq) + Ca 3 (PO 4 ) 2 (s)

364 views • 22 slides

Chemistry 12.1

Chemistry 12.1. 12.1. Interpreting Chemical Equations. A balanced chemical equation can be interpreted in terms of different quantities, including numbers of atoms, molecules, or moles; mass; and volume. 12.1. Interpreting Chemical Equations.

182 views • 18 slides

The Mole

The Mole. Too small to see. Because atoms are so small , it makes more sense to measure large amounts of atoms in reactions . One mole of a substance contains the same number of particles as atoms in 12 grams of Carbon-12. The Avagadro Constant.

248 views • 13 slides

The Mole!

298 views • 11 slides

11:33 PM

page 100. mass. relative atomic or formula mass. 2 x (1+14+16+16+16) = 126g. 0.5 x (40+12+16+16+16) = 50g. 5.4 x (24+16+16+1+1)) = 113g. The number of protons and neutrons the atom contains. 11:33 PM. page 100. no. of moles = mass of chemical molar mass.

209 views • 9 slides

CH 3 OH + O 2 ? CO 2 + H 2 O C= C=

CH 3 OH + O 2 ? CO 2 + H 2 O C= C= H= H= O= O=. 2. 3. 2. 4. 1.5. 2. 2. 2. 8. 8. 8. 8. 1. 1. 2. 4. 4. 3. 4. 4. 3.

199 views • 7 slides

CH 3 OH + O 2 ? CO 2 + H 2 O C= C=

CH 3 OH + O 2 ? CO 2 + H 2 O C= C= H= H= O= O=. 2. 3. 2. 4. 1.5. 2. 2. 2. 8. 8. 8. 8. 1. 1. 2. 4. 4. 3. 4. 4. 3.

190 views • 7 slides