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- 1. S e c t i o n t h r e e B y : Y o u s s ef B e r b ar
- 2. Mole : 6.022 x 10^23 units, the number equal to the number of carbon atoms in exactly 12 g of pure C 12 Molar mass : the mass of one mole of a pure substance. Avogadro no : 6.022 x 10^23
- 3. How to calculate : How to know atomic mass ?! If we have a element that has 2 isotopes and we want to calculate the atomic mass we follow the following rule : Ratio of isotope one * its mass + ratio of isotope 2 * its mass = no its unit is Amu , also it is written under the element symbol in the periodic table Molar mass = Molecular mass = atomic mass in its magnitude
- 4. What is the difference between molar , molecular and atomic mass Both of them are equal in magnitude but the unit of atomic mass is Amu and the unit of molar and molecular mass is g / mole Another example what is the molar mass of co2 : 12 g / mole calculate the molecular mass of water (H2O) (1.01 amu + 1.01 amu + 16.00 amu) = 18.02 Amu or 18.02 g / mole Molar mass of element is no. g / mole . What means ? Molar mass = mass / Avogadro no ( no of moles ) No of moles = mass / molar mass
- 5. Some definitions standard temperature and pressure (STP):standard temperature is 273.15 kelvins and standard pressure is 760 mm Hg ( 1 atm). Stoichiometry : the study of the relationships (mass- mole-volume) among substances involved in chemical reactions. dimensional analysis : a name for “equivalent measures.” A method for solving problems that involves canceling units.
- 6. The equation also shows that 2 mol C8H18 react with 25 mol O2 to form 16 mol CO2and 18 mol H2O. No of mole = mass / molar mass Density = mass / volume
- 7. Problem one
- 8. Solution of problem one Mole ratio = We have 312 moles of ammonia so ,
- 9. Problem two
- 10. Solution of problem two
- 11. Problem Three
- 12. Solution of problem Three
- 13. Problem four
- 14. Solution of problem four
- 15. Thanks for listening Youssef Berbar

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