"Danshui no2" Essays and Research Papers

2 Thermos Thurman 211526893   PRACTICAL 2: Preparation of sodium hexanitrocobaltate (III) Date: 12 March 2014 INTRODUCTION Sodium hexanitrocobaltate (III) is a coordination complex which has the formula Na3[Co(NO2)6]. This compound is yellow in colour. It consists of a central Co3+ ion surrounded by six nitro ligands [1]. This compound is used as a qualitative test for potassium and ammonium ions (so long as certain other cations are not present) [1]. Potassium

Free Ion Mole Oxygen

CH3(g)+Cl2(g)⟶CH3Cl(g)+Cl−(g)(step 2 (fast)) with an elementary rate law of‚ k2=[CH4][Cl2] The steps combine to generate the final reaction equation‚ CH4(g)+2Cl2(g)⟶CH3Cl(g)+HCl(g)+Cl−(g)(overall reaction) Example 2a nsider the following reaction: CO(g)+NO2(g)→CO2(g)+NO(g)(overall reaction) This reaction equation suggests that the carbon monoxide directly reacts with nitrogen dioxide to form the products. However‚ its reaction mechanism shows this is not the case. Consider the two elementary processes below:

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Amanda Tran Date of lab: 04/25/05 Date submitted: 05/09/05 Chem 2130-3 Experiment 3: Synthesis of Co(acac-NO2)3 Introduction In this lab‚ Co(acac·NO2)3 is synthesized using the Co(acac)3 complex produced in Experiment 2. The Co(acac)3 complex is used as a reagent instead of acacH because acacH cannot be directly converted to 3-nitroacetylacetone. Since Co(acac)3 is not stable in HNO3‚ Cu(NO3)2 and acetic anhydride are used in this reaction to produce the final product

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Experiment #10 & #11 The Synthesis of Cobalt Oxalate Hydrate The Synthesis of a Nitrite Complex   February 5‚ 2012   Chemistry 1211L - 146 - Spring 2012   Procedure The Synthesis of Cobalt Oxalate Hydrate Place 100 ml of distilled water in a 250-ml (or 400-ml) beaker. Add 1.26g of oxalic acid dihydrate (H2C2O4.2H2O) and 1 ml of concentrated ammonia. Stir the mixture until the solid has dissolved completely. Dissolve 2.34 g of cobalt chloride hexahydrate (CoCl2.6H2O) in 100 ml of water

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Br Br HNO3 / H2SO4     Mechanism    The first step is the formation of the NO2 from the nitric acid:    NO2 1.3) O O S N HO O O HO O N + H2O + HSO4- OH O     The second step is the nucleophile attack of the bromobenzene on the NO2. The  temperature is moderated to avoid the formation of ortho and meta products:    Br Br O + H+ N O   NO2 2. PROCEDURE    2.1) Reaction    In a 100mL twin‐neck bottom flask a mixture of nitric acid and sulfuric acid was 

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O2(g) 4. Write a balanced chemical equation for the oxidation of Cd(s) by concentrated nitric acid‚ producing NO2(g) and Cd2+(aq). a. HNO3(aq) + Cd(s)  Cd2+(aq) + NO2(g) + OH–(aq) b. 2 HNO3(aq) + Cd(s)  Cd2+(aq) + 2 NO2(g) + 2 OH–(aq) c. HNO3(aq) + Cd(s) + H+(aq)  Cd2+(aq) + NO2(g) + H2O( ) d. 4 HNO3(aq) + Cd(s)  Cd2+(aq) + 2 NO2(g) + 2H2O( ) + 2 NO3–(aq) e. HNO3(aq) + Cd(s)  Cd2+(aq) + NO2(g) Answer Section MULTIPLE CHOICE 1. 2. 3. 4. ANS: ANS: ANS: ANS: E E D D

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76 g(76 %) Introduction Linkage isomers may arise when one or more of the ligands can coordinate to the metal ion in more than one way. The first reported example of linkage isomerism had the formula [Co(NH3)5(NO2)]Cl2.1 This compound exists in two isomeric forms; one containing Co-NO2 linkage‚ the other the Co-ONO group.2 In this experiment‚ the synthesis of both of the isomers will be performed. The figure below illustrates the bonding in nitrito(on the right) and nitro(on the left) Figure

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Engineering Chemistry III Prof. K. M. Muraleedharan Aromatic electrophilic substitution (Ar-SE) Reactions The special reactivity of aromatic systems towards electrophiles arises mainly from two factors: the presence of π electron density above and below the plane of the ring - making it nucleophilic‚ and the drive to regain the aromatic character by opting for substitution as opposed to a simple addition reaction. Preference towards addition reactions in the case of alkenes and substitution

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carbonmethoxy
group
directs
the
nitronium
ion
to
a
position
of
meta.
For
example‚
 formation
of
carbonation
intermediate
yields
a
resonance
stabilized
structure
of
the
 proton.


 
 
 NO2 H3CO O H3CO O H3CO O H3CO O O N O NO2 H NO2 NO2 NO2 H H3CO O H3CO O HSO4 NO2 NO2 H2SO4 
 
 Procedure:

The
procedure
is
outlined
is
“the
laboratory
Manual
for
Organic
 Chemistry
2311”‚
Eight
Edition
by
Jane
E.
Wissinger.
University
of
Minnesota
 Department
of
Chemistry

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Nitration of Methyl Benzoate Abstract: This procedure demonstrates the nitration of methyl benzoate to prepare methyl m-nitrobenzoate. Methyl benzoate was treated with concentrated Nitric and Sulfuric acid to yield methyl m-nitrobenzoate. The product was then isolated and recrystallized using methanol. This reaction is an example of an electrophilic aromatic substitution reaction‚ in which the nitro group replaces a proton of the aromatic ring. Following recrystallization‚ melting point and infrared

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