0
How about such as tablespoon of sugar
or a tablespoon of salt?
How will you determine the number of
particles in a tablesp...
Lorenzo Romano Amedeo
Carlo Avogadro di Quaregna
e di Cerreto,
Count of Quaregna and Cerreto
was an Italian scientist.
He ...
In tribute to him,
the number of
elementary entities
(atoms, molecules, i
ons or other
particles) in
1 mole of a
substanc...
Question:
One mole of cotton has the same number
of particles as one mole of salt.
One mole of an element contains the
same number o...
1 mole = 6.02 ×1023
Multiply 2 by
Avogadro’s number.
1. Atomic mass of C?
2. Atomic masses of
H and O?
3. Atomic masses of
Na and Cl?
One mole of any substance
contains the same number of
particles.
What about the mass of a
mole of a substance?
Is it same ...
The mass of an element or
compound depends on the mass of
its particles.
Therefore, one mole of hydrogen
has a mass depend...
Answer: 12.01 amu
What is the molar mass of
carbon?
The molar mass of carbon is 12.01 g.
How many atoms are I 12.01g of
ca...
The atomic mass of oxygen is
_______. Its molar mass is
_____________. There are ______
atoms found in ________ g of
oxyg...
Number of moles Cl = given mass
molar mas
= 70.9 g
35.45 g/mol
= 2 mol
Number of moles = given mass
molar mass
1. How many moles are there in
6.05 g of carbon?
2. How many moles are there in
46.00 g of sodium?
1. Find the molar mass of water.
a. Multiply the atomic mass of H by 2 and
that of O by 1.
H = 2 x 1.008 = 2.016
O = 1 x 1...
Let’s See What You Have Learned
Α. Determine the molar masses of the
following:
1. acetic acid (CH3COOH)
2. agua oxigenada...
Let’s Remember!
♦ The mole is a unit for counting
particles in a given mass of a
substance. Each mole of a substance
is ma...
The mole concept
The mole concept
The mole concept
The mole concept
The mole concept
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The mole concept

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Transcript of "The mole concept"

  1. 1. How about such as tablespoon of sugar or a tablespoon of salt? How will you determine the number of particles in a tablespoon of salt? Is the number of particles in a tablespoon of sugar the same as the number of particles in a tablespoon of salt?
  2. 2. Lorenzo Romano Amedeo Carlo Avogadro di Quaregna e di Cerreto, Count of Quaregna and Cerreto was an Italian scientist. He is most noted for his contributions to molecular theory, including what is known as Avogadro's law.
  3. 3. In tribute to him, the number of elementary entities (atoms, molecules, i ons or other particles) in 1 mole of a substance, 6.02214179(30)×1023 is known as
  4. 4. Question:
  5. 5. One mole of cotton has the same number of particles as one mole of salt. One mole of an element contains the same number of atoms as a mole of any other element. 1 M of a given element = 1 M of other elements 1 mole of a compound = 1 mole of other compounds
  6. 6. 1 mole = 6.02 ×1023 Multiply 2 by Avogadro’s number.
  7. 7. 1. Atomic mass of C? 2. Atomic masses of H and O? 3. Atomic masses of Na and Cl?
  8. 8. One mole of any substance contains the same number of particles. What about the mass of a mole of a substance? Is it same for all substances?
  9. 9. The mass of an element or compound depends on the mass of its particles. Therefore, one mole of hydrogen has a mass dependent on it atomic mass. - MOLAR MASS MOLAR MASS- the mass in grams that is numerically equal to the atomic mass. The unit of molar mass is grams / mole (g/mol).
  10. 10. Answer: 12.01 amu What is the molar mass of carbon? The molar mass of carbon is 12.01 g. How many atoms are I 12.01g of carbon? 6.022 x 10^23 atoms
  11. 11. The atomic mass of oxygen is _______. Its molar mass is _____________. There are ______ atoms found in ________ g of oxygen. The atomic mass of sodium is _________. Each mole of sodium has a mass of ______. Every ______ g of sodium has _______ atoms.
  12. 12. Number of moles Cl = given mass molar mas = 70.9 g 35.45 g/mol = 2 mol Number of moles = given mass molar mass
  13. 13. 1. How many moles are there in 6.05 g of carbon? 2. How many moles are there in 46.00 g of sodium?
  14. 14. 1. Find the molar mass of water. a. Multiply the atomic mass of H by 2 and that of O by 1. H = 2 x 1.008 = 2.016 O = 1 x 16.00 = 16.00 18.016 or 18.02 Number of moles (H2O) = 36.04 g 18.02 g/mol = 2.0 mol
  15. 15. Let’s See What You Have Learned Α. Determine the molar masses of the following: 1. acetic acid (CH3COOH) 2. agua oxigenada (H2O2) 3. ammonia (NH3) Β. Determine the number of moles in 1. 120.0 g of acetic acid 2. 17.0 g of agua oxigenada 3. 51.0 g of ammonia
  16. 16. Let’s Remember! ♦ The mole is a unit for counting particles in a given mass of a substance. Each mole of a substance is made up of 6.022 × 1023 particles. ♦ The molar mass of a substance is the mass in grams that is numerically equal to the atomic mass or formula mass of the substance.
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