Chemical Equilibrium
DATE PERFORMED: DECEMBER 14, 2010 CHEMICAL EQUILIBRIUM RESULTS AND DISCUSSION Data and Results Table I. The copper-ammonia system # of drops added Color Initial ----- Light Blue Addition of NH3 8 Deep Blue Addition of HCl 9 Very Light Blue Reaction for the copper-ammonia system: Cu2+ + 4NH3 - [Cu(NH3)4]2+ (Pale blue) (Deep blue) According to the Le Châtelier's principle, the addition of excess NH3 to Cu2+ will lead to the formation of a deep blue complex, [Cu(NH3)4]2+ thus giving the solution a deep blue color. The addition of HCl (Cl-) will lead to formation of CuCl2 (consumption of Cu2+) instead of [Cu(NH3)4]2+ because CuCl2 is more stable than [Cu(NH3)4]2+, which will result in a deficiency of Cu2+ and according to the Le Châtelier's principle, the reverse reaction will be favored (formation of more Cu2+) thus giving the solution a light blue color. The data in Table I obtained in the experiment are consistent with the Le Châtelier's principle. Table II. The chromate-dichromate system Well # Reagent Visible Result Net Ionic Equation 1 H2SO4 Yellow-Orange 2CrO42- + 2H+ - C Cr2O72- + H2O 2 NaOH No color
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Synthesis of [Co(NH3)5Cl]Cl2:
Synthesis of [Co(NH3)5Cl]Cl2: Kinetics of Reaction Introduction In this experiment, the substance was tested at on temperature (85 degree Celsius), the rate constant for the substance at 60 degrees Celsius was given, and the remaining temperatures (the other 5) were obtained from a posting of other group's calculations. For the preparation of the compound pentaamminechlorocobalt(III)chloride, compounds [Co(NH3)4CO3]NO3, HCl concentrate, and NH3 concentrate are experimentally combined. The first reason that this experiment is useful is because the compound would in future weeks, be used for following experiments to determine both rate constant and activation energy of pentaamminechlorocobalt(III)chloride. Other reasons to study synthesis and kinetics using hydrolysis would help to determine the behavior of the reaction as being independent or dependent of a base-catalyst 1. Also, by understanding the kinetics of this compound, other, more complex compounds, can be easier to understand. Learning and understanding behaviors of the hydrolysis can help to make better predictions when like compounds react in other similar mixings of compounds 4. Kinetics is the study of motion. In the study of kinetics of the compound being prepared, the H+ ion movement can be determined 3. Having a model of this reaction can be useful in predicting reaction kinetics for similar
Using Volatile Liquids with Set Conditions to Find Molar Mass of an Unknown
Using Volatile Liquids with Set Conditions to Find Molar Mass of an Unknown Erin Lab Performed: October 14th, 2008 Section 006 T.A: Teresa Introduction The purpose of this experiment was to find the molar mass of the unknown substance and compare it to the universal molar masses of different alcohols. This process can be done using the ideal gas law which is pressure and volume is proportionate to number of moles, the universal gas constant and temperature (Department of Chemistry, 2008). Jean Baptiste Dumas, a French chemist whom began his career as a pharmacist and later greatly contributed to modern science. His most well known and accredited work is studying vapour densities of elements which in turn is used to discover their molar masses. However, the scientist did not directly develop the Dumas method because of the nonexistence of the mole at that time. The Dumas method uses the formula M=mRT/PV,M for molar mass, m for mass, R for the universal gas constant, T for temperature, P for atmospheric pressure and V for volume (Sloane, Thomas O'Conor, 1909). Molar mass is the mass of one mole of a substance. The number of moles of a substance is the number of atoms in that element compared to the number of atoms of a carbon-12 molecule. For this experiment we used the ideal gas law. The ideal gas law is all collisions between molecules are free of intermolecular
To identify an unknown compound that has one oxygen atom per molecule, To establish the functional group of the compound, to prepare a derivative and find its melting point, and finally to determine the boiling pont of the original compound.
Identification of an organic compound Aim: To identify an unknown compound that has one oxygen atom per molecule, To establish the functional group of the compound, to prepare a derivative and find its melting point, and finally to determine the boiling pont of the original compound. Plan Establishing the functional group of the compound: To firstly determine the functional group I will carry out Diagnostic tests for functional groups, The test and positive observed reaction is shown below: Functional groupTestPositive resultCarbonylCollect some 2,4-dinitrophenylhydrazine (Brady's reagent) in a dry tube and add a very small amount of the compound and shake.A yellow or orange precipitate forms slowlyAldehydeCollect some silver nitrate solution. Add 2 drops of sodium hydroxide solution, then aqueous ammonia until the mixture is almost colorless. Now add a very small amount to the substance.A grey/black precipitate or silver mirror will be formedKetoneTake some iodine in potassium iodide solution; add sodium hydroxide until it is pale yellow. Add a few drops of compound and shake.A yellow precipitate (iodoform) slowly forms.Primary/secondary alcoholsAdd a small amount of Phosphorus Pentachloride to the compound in a fume cupboard.Steamy fumes of HCl gas are observed, these can be tested with damp litmus paper to confirm acidic gas. After testing
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Synthesis and Characterization of [Co(NH3)4CO3]NO3
Synthesis and Characterization of [Co(NH3)4CO3]NO3 Introduction In this experiment, the main goal is to study the formation and properties of a coordination compound. A coordination compound is composed of a central atom bound to multiple groups called ligands. There is a wide variety of possible ligands that can bond directly to the central atom, but only two common ones, NH3 and CO3, are to be studied in this particular experiment. In the formation of carbonatotetraamminecobalt (III) nitrate, denoted [Co(NH3)4CO3]NO3, the transition metal which serves as the central atom is cobalt. Its first coordination sphere, or everything directly bonded to the cobalt, is four nitrogen atoms and two oxygen atoms. This coordination sphere is represented in the chemical formula with brackets. Because cobalt is involved in six bonds, its coordination number is six, and the structure around the cobalt is octahedral. It is apparent where the four nitrogen atoms come from, since there are three ammonia molecules in the formed complex. However, there is only one carbonate molecule. This ligand is called a bidentate ligand because two of its atoms were bonded to the metal. Thus, the ammonia ligands are all monodentate ligands because only one of their atoms was bonded to the metal. Because the first coordination sphere does not break apart in aqueous solution, it is considered a
Cracking liquid paraffin
James Buthlay Cracking liquid paraffin 03/10/04 In this investigation we set up and experiment to try a figure out what was given off when we 'cracked' liquid paraffin. Cracking is the process of breaking down large, not very useful hydrocarbons and splitting them up into smaller, more useful hydrocarbons. When cracking a hydrocarbon, we always end up with alkanes and at least one alkene. Paraffin can be cracked by passing liquid paraffin vapour over hot pieces of porcelain. The gases released then travel down through a tube into a test tube where they are bottles and collected. These are the gases in which we are trying to identify. The first test to try and identify what we had collected in the test tube, was a test for hydrogen. This was a simple test and simply involved putting a lighted splint into the test tube. If a 'pop' occurred then hydrogen was present and the splint would be extinguished. If no hydrogen was present, nothing happens. The outcome of this test was as follows: Test tube number Observations Conclusion Nothing happened No hydrogen present 2 Nothing happened No hydrogen present 3 Nothing happened No hydrogen present 4 Slight 'pop' noise Little hydrogen present 5 Louder 'pop' Hydrogen present 6 'pop' and flame Hydrogen present 7 'pop' and flame Hydrogen present 8
Heat Capacity Ratio for Gases. The experimental heat capacity ratio of N2 gas is computed as 1.28 (0.02) with the help of the adiabatic expansion method. This value is closer to the theoretical value of 1.29 when vibrational contribution to Čv is
Heat Capacity Ratio for Gases V. Raw and Derived Data Tables: Table 1: Manometer Readings for PNitrogen Gas in the Carboy Trial Height 1 (cm) Height 2 (cm) ?H (cm methyl salicylate) ?H (mm Hg) [P1] (mmHg) 31.90 ± 0.05 49.90 ± 0.05 8.00 ± 0.07 5.60 ± 0.06 770.85 ± 0.26 2 7.40 ± 0.05 64.10 ± 0.05 46.70 ± 0.07 40.46 ± 0.06 795.71 ± 0.26 3 24.30 ± 0.05 57.60 ± 0.05 33.33 ± 0.07 28.85 ± 0.06 784.10 ± 0.26 Table 2. Manometer Readings for PNitrogen Gas in the Carboy after the Cap was removed and Subsequently Plugged Trial Height 1 (cm) Height 2 (cm) ?H (cm) ?H (mm Hg) [P3] (mm mercury) 38.90 ± 0.05 42.90 ± 0.05 4.00 ± 0.07 3.47 ± 0.06 758.72 ± 0.26 2 36.20 ± 0.05 45.70 ± 0.05 9.50 ± 0.07 8.23 ± 0.06 763.48 ± 0.26 3 37.30 ± 0.05 44.40 ± 0.05 7.10 ± 0.07 6.15 ± 0.06 761.40 ± 0.26 Table 3. Mean Heat Capacity Ratio Trial Heat Capacity Ratio Mean Heat Capacity Ratio SD ku .29 ± 0.05 .28 ± 0.02 0.01 0.02 2 .26 ± 0.02 3 .28 ± 0.03 Table 4: Theoretical Cp and CV of Nitrogen gas CP (J mol-1 K-1) CV (J mol-1 K-1) Without vibrational With vibrational Without vibrational With vibrational 29.099 37.413 20.785 29.099 Table 5: Heat Capacity Ratio of N2 (Experimental and Theoretical) Experimental Heat Capacity Ratio Theoretical Heat Capacity Ratio Error (%) Without vibrational With
Ionic Reactions Experiment.
Ocean County College Department of Chemistry Lab #8- Ionic Reactions Submitted By, Stephen Gorda Date Submitted: 3-26-12 Date Performed: 3-27-12 Lab Section: Chem-181DL1 Course Instructor: Prof. Maria Tamburro Purpose This lab experiment will provide the experimenter with an opportunity to understand the nature of ionic reactions. This experiment will show how these reactions occur by giving examples of reactions, such as precipitation reactions, and breaking down these reactions by use of equations to see the net ionic reaction. This lab provides the unique opportunity to not only predict ionic reactions, but also see them through experimentation. A better understanding of balanced equations, solubility rules, aqueous solutions, and ionic reactions in general will most likely be better understood upon completion of this experiment (LabPaq CK-1). Procedure . I first read through entire procedure and then set up lab area. 2. I obtained a light and dark sheet of paper to view reactions against both a light and dark
The objective of this experiment is to determine how a buffer system resists large changes in pH due to addition of strong acids.
SINGAPORE POLYTECHNIC SCHOOL OF CHEMICAL LIFE SCIENCES Diploma of Applied Chemistry with Pharmaceutical Science Experiment 4 Measurement of pH and Determination of Buffer Capacity CP4120 Desmond Seah (P1006812) Year of Study: Year 1 DACP/FT Lecturer Joseph Chan AY 10/11 ________________ Content Page Synopsis Page . Objectives of Experiment 1 2. Theory 1 2.1 Buffers and pH calculation 1-5 2.2 Water a Poor Buffer 5-6 2.3 Instrument – Glass Electrode pH meter 6-8 . Procedure 9 2. Results and calculation 9-10 3. Discussion 11-12 5.1 Instrument Errors
The two central objectives of this experiment are the production of Aspirin from esterification of salicylic acid with excess acetic anhydride and obtaining it in a purer state by recrystallisation
SINGAPORE POLYTECHNIC SCHOOL OF CHEMICAL LIFE SCIENCES Diploma of Applied Chemistry with Pharmaceutical Science Experiment 2 Preparation of Recrystallization of Aspirin CP4120 Desmond Seah (P1006812) Year of Study: Year 1 DACP/FT Lecturer Lim Lee Yee AY 10/11 ________________ Content Page Synopsis Page . Objectives of Experiment 1 2. Introduction 1-2 3. Theory 2-4 4. Procedure 5 5. Results and calculation 5-6 6. Discussion 6-7 7. Conclusion 7 8. Recommendation References List of Illustration S/N Figures and Tables Page Number Recrystallised aspirin iii 2 Baeyer Hoffman 1 3
