sch3u_unit3_review.pdf

# sch3u_unit3_review.pdf - SCH3U Unit 3 Quantities in...

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SCH3U Unit 3: Quantities in Chemical Reactions Review Sheet Important equations: 1. Calculate the following: a) How many moles are present in 8.5 g of magnesium nitrate, Mg(NO 3 ) 2 ? b) How many atoms are there in 8.5 g of Mg(NO 3 ) 2 ? c) How many moles are there in 4.20 x 10 21 molecules of methane? d) What is the mass of 1.0 x 10 23 molecules of water? 2. Titanium reacts with oxygen to produce titanium oxide, the pigment that gives paint and sunscreen a white colour. . a) If 15.6 g of titanium reacts with oxygen to form 20.0 g of titanium oxide, calculate the mass of oxygen that reacted. What chemistry law are you using? b) Calculate the percent composition of titanium oxide. b) How much titanium oxide can be produced from 500 g of titanium and unlimited oxygen? What law are you using to solve this? 3. What is the percent composition of: a) sodium carbonate (Na 2 CO 3 )? b) aluminum oxide (Al 2 O 3 )? 4. What is the empirical formula of a compound that is: a) 30.4% N, 69.6% O (by mass) b) 43.6% P, 56.4% O (by mass) 5. What is the molecular formula of a compound with molar mass 60.0 g and composed of 39.97% C, 6.73% H, and 53.30% O (by mass)? The mole and molar mass There are 6.02 x 1023 particles in one mole Molar mass is calculated from PT # of particles Mole Mass and Mass Mole # of Particles Percentage composition (Element mass ÷ Compound mass ) x 100% Empirical and Molecular Formula Determine simplest formula from % composition, grams of reactants, or moles Calculate molecular formula from simplest formula and molar mass Stoichiometry grams A moles A

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