0 hydrogen peroxide solution in Jg o C 4184 4184 n Amount of heat gained in

0 hydrogen peroxide solution in jg o c 4184 4184 n

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m) Specific heat of a 3.0% hydrogen peroxide solution in J/(g o C): 4.184 4.184 n) Amount of heat gained (in Joules) by 3.0% hydrogen peroxide solution : o)Amount of heat lost (in Joules) by the hydrogen peroxide reacting (or heat of reaction) †† : p) Amount of heat lost (in kilojoules) by the hydrogen peroxide reacting (or heat of reaction) (o/1000): q) Enthalpy of reaction (in kilojoules per mole) for the decomposition of hydrogen peroxide(p/f): r) Average enthalpy of reaction (inkilojoules per mole) for the decomposition of hydrogen peroxide((q 1 +q 2 )/2): q = ( s m Δ t ) Experiment #11A Barnett †† q solution = – q reaction
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61 Table #2: Sample Data Table the Heat of Reaction by Bond Energy: Lewis Dot Diagram Lewis Dot Diagram Lewis Dot Diagram H 2 O 2 ( aq ) Fe(NO 3 ) 3 H 2 O( l ) ½ O 2 ( g ) Data Recorded/Calculated Data a) Sum of bonds broken* (in kJ/mol): b) Sum of bonds formed* (in kJ/mol): c) Enthalpy of reaction (in kJ/mol) for the decomposition of hydrogen peroxide via BE (a – b): Table #3: Sample Data Table for the Enthalpy of Reaction via Hess’s Law: Data Recorded/Calculated Data a) Known reaction #1: H2(g) + O2(g) barb2rightH2O2(aq)∆Hf= –191.2 kJ/mol b) Known reaction #2: H2(g) + ½ O2(g) barb2rightH2O(l)∆Hf= –285.8 kJ/mol c) Unknown reaction: H2O2(aq) barb2rightH2O(l) + ½ O2(g)∆Hrxn= _____________ Table #4: Sample Data Table for the Enthalpy of Reaction Comparison: Data Recorded/Calculated Data a) True enthalpy of reaction (in kJ/mol) for the decomposition of hydrogen peroxide via Hess’s Law: Via Calorimetry Via Bond Energy b) Experimental enthalpy of reaction (in kJ/mol) for the decomposition of hydrogen peroxide: c) Percent error (%): d) Which method is more accurate?* *Select from “Via Calorimetry” or “Via Bond Energy” *Use information from Table A from the “Introduction to Bond Energy” section Experiment #11A Barnett
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Experiment #12: Electron Pair & Molecular Geometry Introduction to VSEPR : 1) The valence – shell electron – pair repulsion model ( VSEPR ) can predict the shape of molecules and ions by proposing that valence–shell electron pairs are arranged about each atom such that these pairs are as far away from one another as possible to minimize electron–pair repulsions. 2) Electron pair geometry is the shape that is obtained by assuming the electron pairs are groups around the central atom. a. There are only five types of electron pair geometry: i. Linear – two groups around central atom ii. Trigonal planar – three groups around central atom iii. Tetrahedral – four groups around the central atom iv. Trigonalbipyramidal – five groups around the central atom v. Octahedral – six groups around the central atom 3) Molecular geometry is the shape that is obtained by assuming the electron pairs are absent around the central atom. a. There are multiple types of molecular geometries depending on the number of bonding groups (or substituents) and the number of loan pairs.
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  • Spring '19
  • Chemistry, Chemical reaction, Timothy Barnett

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