takes precedence (a) V2O5 (1) (b) ZnSO4 (1) (c) AgI (1) (d) CF3Cl3 (1) (e) (NH4)2SO4 / ZnSO4 (1) (f) CH4 (1) (g) (NH4)2SO4 (1) [1] [1] [1] [1] [1] [1] [1] [Total: 7] A2 (a) sulfur dioxide (1) Allow SO2 (b) copper(II) sulfate (1) Allow CuSO4 (c) H+ + OH– → H2O (1) Ignore state symbols (d) (i) Copper(II) hydroxide (1) Allow Cu(OH)2 (ii) Cu2+(aq) + 2OH–(aq) → Cu(OH)2(s) Balanced equation (1) Correct state symbols (1) [1] [1] [1] [1] [2] (e) Mol ratio Cu:O = CuO (1) 79.9 20.1 : / 1
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between (n-1)d &ns orbital as a result both (n-1)d &ns electrons take part in bond formation. The highest oxidation state of an element is equal to number of unpaired electrons present in (n-1)d &ns orbital. Transition elements have high enthalpy of atomization/ sublimation Because of large number of unpaired electrons in their atoms‚ they have stronger interatomic interaction and hence strong metallic bonding is present between atoms. Most of transition elements are paramagnetic due
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Lab #6 Properties of Hydrates Purpose: The purpose of the “Properties of Hydrates” lab is to study hydrates‚ and be able to identify them. This lab also focuses on observing the reversibility of hydration reactions by hydrolysis‚ and also testing substances for efflorescence of deliquescence. Procedure: A. Identification 1. Place 0.5 grams of each compound (Nickel Chloride‚ Potassium Chloride‚ Sodium Tetraborate‚ Sucrose‚ Calcium Carbonate‚ and Barium Chloride) in a small dry test
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Chem 16 Notes UPD Should only be a supplement to discussions Table of Contents* [A] Lecture [1] Thermodynamics [2]Energy [3]Enthalpy [4]Hess’s Law [5]Determining Enthalpy [6]Heat Capacity [7]Calorimetry [8] Entropy [9] Gibb’s Free Energy [10] Waves [11] Quantum Theory [12] Quantum Numbers [13] Electron Configuration [14] Periodic Table [15] Periodic Trends KSev [16] Chemical Bonding [17] Formal Charge [18] Resonance Structure [19] Bonds [20] VSEPR [22] Valence Bond Theory [22] Molecular Orbital
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dissolve exothermically in water. The enthalpy change of solution‚ ΔHsoln‚ is the energy change associated with the following reaction. M represents the Group I metal. M +(aq) + OH–(aq) M OH(s) + (aq) The following diagram represents theoretical stages in the formation of aqueous MOH. M +(g) + OH-(g) + (aq) lattice energy hydration enthalpy of the ions H hydration M OH(s) + (aq) H soln M +(aq) + OH-(aq) Lattice energy and hydration enthalpy are both more exothermic when ions
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along with alkalies and minor amounts of other elements Hydration. The most important hydraulic constituents are the calcium silicates‚ C2S and C3S. Upon mixing with water‚ the calcium silicates react with water molecules to form calcium silicate hydrate (3CaO 2SiO23H2O) and calcium hydroxide (Ca [OH] 2). These compounds are given the shorthand notations C-S-H (represented by the average formula C3S2H3) and CH‚ and the Hydration reaction can be crudely represented by the following reactions:
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following will be least soluble in water? A. potassium sulfate‚ K2SO4 B. ammonium nitrate‚ NH4NO3 C. chloromethane‚ CH3Cl D. calcium chloride‚ CaCl2 E. ethanol‚ C2H6O 3. Select the precipitate that forms when the following reactants are mixed. Mg(CH3COO)2(aq) + LiOH(aq) A. LiCH3COO B. Li(CH3COO)2 C. MgOH D. Mg(OH)2 E. CH3OH 4. Select the precipitate that forms when aqueous lead(II) nitrate reacts with aqueous sodium sulfate. A. NaNO3 B. Na2NO3 C. PbSO4 D. Pb2SO4 E. PbS
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description of an experimental determination of the enthalpy of reaction of sulfuric acid in a reaction with magnesium to produce magnesium sulfate. Through the use of an ice calorimeter‚ the rxn H° D for this reaction is determined to be 1 360kJ mol − − × . Introduction: This report details an experiment in thermochemistry. Included are the methods‚ results‚ and interpretation of results of an experimental determination of an enthalpy of reaction. The reaction being studied is between sulfuric
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percent yield (i.e. CuSO4 was obtained from the reaction of CuO with sulfuric acid. If 2.5 g of CuSO4 was obtained from 5.0 g of CuO‚ what is the percent yield?) Purpose To observe the chemical properties of copper through a series of reactions To recover the original mass of solid copper by synthesizing different
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the experiment is to analyze alum‚ AlK( SO4 )2 . 12 H2 O‚ by three techniques in order to verify its identity. The following properties will be determined namely‚ melting point‚ mole ratio of hydrated water to anhydrous alum‚ and percent of sulfate ion contained in the compound. Each of these properties will be compared to the literature or established values for alum. In this experiment‚ the first step ( Part 1 ) is to find the melting point of the compound and compare it to the published
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