1 mol 1 mol molar mass 6.02 × 1023 Mass (g) Particles (atoms, molecules, formula units) 18. How many moles are in 34.5 g of water? 19. How many molecules are in 0.456 moles of water? 20. How many moles are in 21.1g of calcium chloride? 21. How many moles are in 6.789 × 1022 formula units of calcium chloride? 22. How many atoms are in 99.99g of nitric acid, HNO3? 23. What is the mass, in grams, of 7.87 × 1025 molecules of sulfur trioxide? Empirical and Molecular Formulas What’s the difference? A molecular formula is the true formula for a substance, for example, tetraphosphorous decoxide is P4O10. An empirical formula has the coefficients reduced down to their lowest possible ratio, for example, that P4O10 can be reduced to P2O5. 24. the empirical formula for the following substances. If it already is an empirical formula, let it be! a. b. C3H8 c. C6H12O6 d. Co2(CO3)3 Stoichiometry determining how much product can be made from a specific amount of – reactants. It is based on the law of conservation of mass and uses MOLE RATIOS to convert between substances! Mole = moles of unknown moles of given If you want to see a step by step procedure for doing stoichiometry, please go to your notes or the following Limiting and Excess reactants Limiting reactants control how much product can be made during a chemical reaction because you run out of that reactant first! An excess reactant is one in which you have more than enough for the reaction to run to completion. Use the balanced equation to answer the following questions: 3 K (s) + Au(NO3)3 (aq) Au (s) + 3 KNO3 (aq) How many of potassium nitrate are produced from 21.0 moles of potassium? How many grams of gold are produced from the reaction of 1.50 moles of potassium with excess gold (III) nitrate? What is the mass, in grams of potassium nitrate produced from the reaction of 50.00g of gold (III) nitrate with excess potassium?
1 mol 1 mol molar mass 6.02 × 1023 Mass (g) Particles (atoms, molecules, formula units) 18. How many moles are in 34.5 g of water? 19. How many molecules are in 0.456 moles of water? 20. How many moles are in 21.1g of calcium chloride? 21. How many moles are in 6.789 × 1022 formula units of calcium chloride? 22. How many atoms are in 99.99g of nitric acid, HNO3? 23. What is the mass, in grams, of 7.87 × 1025 molecules of sulfur trioxide? Empirical and Molecular Formulas What’s the difference? A molecular formula is the true formula for a substance, for example, tetraphosphorous decoxide is P4O10. An empirical formula has the coefficients reduced down to their lowest possible ratio, for example, that P4O10 can be reduced to P2O5. 24. the empirical formula for the following substances. If it already is an empirical formula, let it be! a. b. C3H8 c. C6H12O6 d. Co2(CO3)3 Stoichiometry – determining how much product can be made from a specific amount of reactants. It is based on the law of conservation of mass and uses MOLE RATIOS to convert between substances! Mole = moles of unknown moles of given If you want to see a step by step procedure for doing stoichiometry, please go to your notes or the following Limiting and Excess reactants Limiting reactants control how much product can be made during a chemical reaction because you run out of that reactant first! An excess reactant is one in which you have more than enough for the reaction to run to completion. Use the balanced equation to answer the following questions: 3 K (s) + Au(NO3)3 (aq) Au (s) + 3 KNO3 (aq) How many of potassium nitrate are produced from 21.0 moles of potassium? How many grams of gold are produced from the reaction of 1.50 moles of potassium with excess gold (III) nitrate? What is the mass, in grams of potassium nitrate produced from the reaction of 50.00g of gold (III) nitrate with excess potassium?
Spring-2015-Honors-Chemistry-Final-Review.docx