APAP化学化学- -物质的结构物质的结构1.1 Relative massAl2O3 K2Cr2O7 H2SO4 HNO3HF CO32-CuSO4 NH4+Fe3O4 P2O51.2 Mole and the Avogadro constantFe=56; H=1; L=6Fe=56; H=1; L=610102323molmol-1-1; V; Vmm=22.4dm=22.4dm3 3/mol/mol 1. How many moles of atoms are contained in 5.6g of iron? 2. How many iron atoms are there in 0.1 mole iron?3. How many moles of 121023 molecules of H2?4. How many molecules are there in 2 moles H2?5. Calculate the volume of 0.2 mole of gas at s.t.p.6. Calculate the moles of 13.44 dm3 of gas at s.t.p.Calculate the volume and mass of 241023 molecules of NH3 at s.t.p. In 36g water, H=1; O=16; L=H=1; O=16; L=6106102323molmol-1-1 (1) how many moles of (1) how many moles of moleculesmolecules are present? are present?(2) how many (2) how many moles of moles of hydrogen atomshydrogen atoms are present? are present?(3) how many (3) how many moles ofmoles of oxygen oxygen atoms atoms are present?are present?(4) how many moles of (4) how many moles of atoms atoms are present?are present? Ethanol has molecular formula C2H5OH. A sample of ethanol has a mass of 2.3 g.(1) How manyHow many moles moles of moleculesof molecules are present ?(2) How many moleculesmolecules are present?(3) How many moles moles of hydrogen atomsof hydrogen atoms are present?(4) How many hydrogen atomshydrogen atoms are present?The sample was completely burnt in oxygen.(5) Write down a balanced equation for the combustion.(6) How many molesmoles of water moleculesof water molecules were produced in the combustion?(7) What massmass of the carbon dioxidecarbon dioxide was produced?(8) How many oxygen molecules oxygen molecules were used up?1.3and1.4 Mass spectra of atoms and molecules1.3and1.4 Mass spectra of atoms and molecules1.5 and1.6 Empirical and Molecular Formulae1.5 and1.6 Empirical and Molecular Formulae(a) Use the value of the Avogadro constant to calculate the total number of atoms in 7.10g of chlorine atoms.(b) Calculate the amount in moles of nitric acid,HNO3, in 25cm3 of a 0.1 mol dm-3 aqueous solution.(c) Calculate the concentration in mol dm-3 of sodium hydroxide, NaOH, if 250 cm3 of a solution contains 2.0g of NaOH.(d) What is the concentration in mol dm-3 of an aqueous solution containing 4.00g dm-3 of sodium hydroxide, NaOH?(e) Calculate the volume, in dm3, occupied by 26.4g of carbon dioxide at room temperature and pressure. Given that at room temperature and pressure, 1 mole of any gas occupies a volume of 24 dm3.Chapter 1 ReviewMultiple ChoMultiple Choi ice Questions:ce Questions:Which of these samples has the largest mass ? A. 2.24 dm3 of ethane,C2H6 . B. 3.61022 molecules of O2.C. 672 cm3 of carbon dioxide CO2.D. 0.05 mole of hydrogen fluoride,HF.Free Response Questions1. An organic compound has the following percentage composition by mass: 40of carbon, 53.33of oxygen and 6.67of hydrogen. The relative molecular mass of the compound is 180. Find the empirical formula and the molecular formula of the compound. 2. 2. 20cm 20cm3 3 of gaseous hydrocarbon was mixed with of gaseous hydrocarbon was mixed with 100cm100cm3 3 of oxygen of oxygen and the mixture sparked so that the hydrocarbon was completely and the mixture sparked so that the hydrocarbon was completely burnt. The volume of gas remaining at the end of combustion was burnt. The volume of gas remaining at the end of combustion was 70 cm70 cm3 3. After passing over soda lime, this volume was reduced to . After passing over soda lime, this volume was reduced to 10cm10cm3 3. All gases were measured at room temperature and at the . All gases were measured at room temperature and at the same pressure. same pressure. Deduced the formula of the hydrocarbon and find the relative molecular mass of the hydrocarbon.Test1. How many atoms are present in 8.8g of carbon dioxide, CO2?2. Calculate the number of atoms of 8g methane,CH4.3. Calculate the number of atoms of 15.6g of benzene, C6H6.4. Calculate the number of atoms of 21.8g of bromoethane, C2H5Br.