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MORE MOLAR MASS PRACTICE…. (NH 4 ) 3 PO 4. HNO 3. Nitric Acid. Ammonium Phosphate. g element. x 100. mass % of element =. molar mass of compound. :. :. :. :. percentage composition : the mass % of each element in a compound. Find the % composition of ammonium phosphate.

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## HNO 3

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**MORE MOLAR MASS PRACTICE…**(NH4)3PO4 HNO3 Nitric Acid Ammonium Phosphate**g element**x 100 mass % of element = molar mass of compound : : : : percentage composition: the mass % of each element in a compound Find the % composition of ammonium phosphate. (NH4)3PO4 42.03 g N = 28.18% N 149.12 g 12.12 g H 149.12 g = 8.13% H 30.97 g P = 20.77% P 149.12 g = 42.92% O 64.00 g O 149.12 g**Different Types of Formulas**C6H6 • Molecular Formula – shows # of atoms in one molecule or formula unit • Empirical Formula – shows smallest whole number mole ratio • Structural Formula- molecular formula info PLUS bonding electrons and atomic arrangement CH All different types of formulas for the same compound…benzene!**Finding an Empirical Formula from Experimental Data**1. Find mass of each element (grams) 2. Find mols of each element (convert from grams to mols) 3. Divide each “# of mol” by the smallest “# of mol” (ratios) 4. Write out formula with ratios from step 3 as subscripts (multiply by smallest integer possible for whole #’s if needed) PRACTICE... A compound is 45.5% yttrium and 54.5% chlorine. Find its empirical formula. YCl3**A ruthenium/sulfur compound is 67.7% Ru.**Find its empirical formula. RuS1.5 Ru2S3**(Empirical Formula)n = Molecular Formula**To find molecular formula… A. Find empirical formula. B. Find mass of empirical formula. C. Find n = Molar Mass molecular empirical mass D. Multiply all parts of empirical formula by n. “How many empiricals fit into the molecular?”**A carbon/hydrogen compound is 7.7% H and has a**molar mass of 78 g. Find its molecular formula. emprical formula = CH Empirical mass = 78 g n = C6H6 13 g = 6 13 g**92 g**46 g A compound has 26.33 g nitrogen, 60.20 g oxygen, and molar mass 92 g. Find molecular formula. ÷ 1.879 ÷ 1.879 Empirical formula = NO2 N2O4 MMempirical = = 2 n = 46 g**Review Problems**A 17.40 g sample of a technetium/oxygen compound contains 11.07 g of Tc. Find the empirical formula. TcO3.5 Tc2O7**Review Problems**A compound contains 70.35 g C and 14.65 g H. Its molar mass is 58 g. Find its molecular formula. emp. form. C2H5 58 g n = C4H10 MMemp= 29 g = 2 29 g**Review Problems**A compound contains 4.63 g lead, 1.25 g nitrogen, and 2.87 g oxygen. Name the compound. PbN4O8 ? ? lead (IV)nitrite Pb(NO2)4 (plumbicnitrite) Pb? 4 NO21–**LET’S REVIEW…**# of H2O molecules # of H atoms # of O atoms 1 2 3 100 6.02 x 1023 2 1 4 2 6 3 200 100 2 (6.02 x 1023) 6.02 x 1023 molar mass: the mass of one mole of a substance 18.0 g 2.0 g 16.0 g**part**whole % = x 100 % QUICK SUMMARY 6.022x1023 Molar Mass vs. Atomic Mass 2 g H2 = _____ H2 = _______ 2 amu 18 g H2O = _____ H2O = ________ 18 amu 120 g MgSO4 = _____ MgSO4 = ________ 120 amu 149 g (NH4)3PO4 = _____ (NH4)3PO4 = ________ 149 amu Percentage Composition Empirical Formula • % g • g mol • mol • mol Empirical vs. Molecular Formula (lowest ratio)

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