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The document discusses mole calculations including mole-mole, mole-mass, mass-mass, mole-molecule, and mass-molecule conversions. It also covers gas stoichiometry problems, determining empirical and molecular formulas, and calculations involving limiting reagents and percent yield. Sample problems are provided for each type of calculation to demonstrate how to determine the number of moles, grams, or molecules of reactants and products.
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캐미 Ppt
- 1. By Keonho Kim, Sanggu Lee
- 2. What is mole? The mole mass is depends on how many electrons are in each atom. For example; H has a mass of 1.01, O has mass of 16. H has less electrons than what O has, so the mass of the H is less than O, also we could find that Mole mass is depends on electron
- 3. What is atomic mass and molar mass? Atomic mass - It is approximately equivalent to the number of protons and neutrons in the atom. Molar mass - The molar mass is a physical property. It is defined as the mass of a given substance divided by its amount of substance.
- 4. Conversions Mole - Mole Mole - Mass Mass - Mass Mole - Molecule Mass - Molecule Mixed: Mole - Mass - Molecule Mole - volume Mass - volume
- 5. Mole - Mole 2H2+O2 → 2H2O How many moles of H2 are required to make 10 moles of water? H2O mole mass 1 H2 mole mass 16.04 1 1.01 10 160.4 x 10.1 x = 10
- 6. Mole - Mass 2H2+O2 → 2H2O How many grams of water can be made with 8 moles of oxygen? H2O mole mass O2 mole mass 1 16.04 1 6 8 x 8 48 To find x we need to do cross multiply. x = 128.32
- 7. Mass - Mass 2H2+O2 → 2H2O How many grams of water can be made with 76g of Oxygen? H2O O2 mole mass 1 16.04 8 x x = 42 mole mass 1 6 12.6 76
- 8. Mole - Molecule 2H2+O2 → 2H2O How many moles of H2O are formed from 8.038*1023 molecules of O2 O2 mole molecule 1 6.023x1023 8.038x1023 x= H2O mole molecule 2 6.023x1023 x
- 9. Mass - Molecule 2H2+O2 → 2H2O How many Molecule of O2 when H2O has a mass of 57.5 O2 H2O mole mass molecule mole mass molecule 1 32 1.20E24 1.90E24 2 36.4 1.20E24 57.5
- 10. Mixed :Mole - Mass - Molecule 2H2+O2 → 2H2O How many mole and mass of O when a H2O has a molecule of 6.5 X 1023 O H2O mole mass molecule mole mass molecule 32 6.023*1023 2 36.02 1.2*1023 1 5.4 173.3 3.26*1024 6.5*1023
- 11. Mole - Volume How many moles of argon atoms are present in 11.2 L of argon gas at STP? Answer 0.5 mole Because 1 mole of any gas is 22.4 at STP. So it is 0.5 mole.
- 12. Mass - Volume How many mass of Hydrogen atoms are present in 50 L of gas at oxygen? H mass volume 1.01 11.2 x Answer- 2.25 O2 mass volume 32 22.4 50
- 13. Gas Stoichiometry? Remember? 2Na(s) + 2H2O(I) → H2(g) + 2NaOH(aq) How many grams of sodium metal are needed to give 7.81g of hydrogen by this reaction? Na mole mass 2 45.98 H mole mass 1 x x = 178g Na 2.02 7.81
- 14. Gas Stoichiometry? Remember? 2Na(s) + 2H2O(I) → H2(g) + 2NaOH(aq) How many molecule sodium water are needed to react with 1.25*10 24 molecules of water? Na H2O mole molecule mole molecule 2 1.20E24 x 2 1.2046E24 1.25E24 x = 1.25 x 10E24 atoms Na
- 15. Empirical and Molecular formula A 20g sample of a hydrate of nickel sulfate (NiSO4) lost 9.63g of water when heated. Determine the hydrate’s formula.
- 16. Percent yield and Limiting reagent Methane, CH4, burns in oxygen to give carbon dioxide and water according to the following equation: CH4 + 2 O2 ------> CO2 + 2 H2O a mixture of 0.350mol of methane was burned in 3mol of oxygen in a sealed steel vessel. Find the limiting reactant, if any, and calculate the theoretical yield, (in moles) of water. 1 mol CH4 = 2 mol O2 If we use up all the methane then: 1 mol CH4 = 2 mol O2 0.350 mol x x = 0.70 mol of O2 would be needed.
- 17. continue If we use up all the oxygen then 1 mol CH4 = 2 mol O2 x 3 mol x = 1.5 mol of methane. We don't have 3 moles of methane. We have only 0.35 moles. Therefore the methane will be used up before all the oxygen is. Again the methane is the limiting reactant. We now use the limiting reactant to make the mole comparison across the bridge to find the amount of water produced. 1 mol CH4 = 2 H2O 0.25 mol x x = 0.70 mol of H2O would be produced. When 0.35 mole of methane and 3 mole of oxygen are mixed and reacted according to the equation, the methane is the limiting reactant and the maximum yield of water will be 0.70 moles.