The resulting material is heated with silica (SiO2) in flash smelting to remove the iron as slag. 2 CuFeS2 + 3 O2 → 2 CuS + 2 FeO + 2 SO2 FeO + SiO2 → FeSiO3 (slag) The copper matte (CuS) produced contains high concentration of copper, the sulfur is removed by blowing air through the molten matte. CuS + O2 → Cu + SO2 2 CuS + 3 O2 → 2 CuO + 2 SO2 This product is 98% pure copper but due to the broken surface created by the escaping sulfur dioxide gas, it is known as blister copper. To remove the oxygen, natural gas is blown through the molten copper oxide, and oxygen is burned off. The copper is then fed to electrolysis for refining.
When the solution is acidified during diazotization to form nitrous acid, the sulfanilic acid is precipitated out of solution as a finely divided solid, which is immediately diazotized. The finely divided diazonium salt is allowed to react immediately with dimethlaniline in the solution in which it was precipitated. Mechanism Diazotization: [pic] Diazo Coupling: Methyl orange is often used as an acid-base indicator. In solutions that are more basic than pH 4.4, methyl orange exists almost entirely as the yellow negative ion. In solutions that are more acidic than pH 3.2, it is protonated to form a red dipolar ion.
Background: Sulfuric acid (H2SO4) is a diprotic acid (can donate 2 protons to a base). Sulfuric acid ionises in water in two stages: HSO4-(aq) + H2O(l) SO42-(aq) + H3O+(aq) H2SO4(l) + H2O(l) -----> HSO4-(aq) + H3O+(aq) Sulfuric acid is a strong acid (complete dissociation in water, Ka approaches infinity). Sulfuric acid reactions: Sulfuric acid + metal
When aqueous zinc nitrate is reacted with a limited amount of potassium hydroxide, insoluble zinc hydroxide forms. 2 [pic] + [pic] [pic] Zn[pic] [Eq. 1] Zinc hydroxide behaves as a base when it reacts with acids to form salts and water. In a solution containing excess [pic] ions, Zn[pic] acts like an acid and dissolves forming the complex ion[pic]. 2 [pic] + Zn[pic] [Zn[pic]][pic] [Eq.
Chemistry Lab Types of Chemical Reactions OBSERVATION DATA TABLE Step|Name of Reactants|Description of Reactants|Description of reaction taking place (evidence of chemical reaction)|Description of Products| 1|Zn|Solid, small chunky bits, Silvery-grey, dull|As the Zinc and Sulfur heated up it expanded in the test tube and shot out Zinc Sulfide.-light and heat are produced|White powder was created and the leftovers of the reactions was a black powder.| |S|Solid, resembles powder, Off-yellowOpaque||| 2|KI|-dull yellow liquid-transparent|Instantaneously changed colour to a bright yellow.|-Bright yellow liquid-Opaque| |Pb(NO3)2|-liquid, transparent, very clear-bubbly||| 3|H2O2|-liquid-clear-transparent|A dark grey bubbling liquid was created. It got hotter as it reacted.gas test observations:The splint relit. Oxygen was present.|Oxygen gas was created and a dark grey opaque liquid was left behind in the test tube. | |MnO2|-solid-powder-black||| 4|AgNO3|A clear, transparent liquid.|As the copper reacted with the Silver Nitrate, the ball of Copper changed colour to grey and subsequently developed a ‘furry-like’ characteristic on its coating.|-Clear liquid-Copper changes to a grey colour, ‘furry-like’.| |Cu|-brown/red-solid-stringy||| 5|HCl|A clear, transparent liquid.|When the Magnesium was inserted the HCl liquid started to bubble and fizz releasing Hydrogen. The Magnesium strip dissolved in the process and the test tube got hotter.
Title : Reaction of Carboxylic Acids Objective : To Determine The Reaction of Carboxylic Acids Procedure : As referred to Lab manual. Results: A. Salt Formation |Compound |Solvent |Solubility | |Benzoic Acid |Cold Water |Partially soluble | |Benzoic Acid |10 % NaOH |Soluble | B. Salt Hydrolysis Sodium acetate solution changed the color of litmus from red to blue. C. Reaction With Sodium Carbonate Observation : A lot of gas bubbles was released.
Name: Amandeep Sandhu |Date: 06/16/2012 | | |Exp 4: Physical & Chemical Properties |Lab Section: | Data Table: Substance |Color |Odor |Effect of Heat |Cold H2O |Hot H2O |Litmus Test |Dilute HCl |Dilute NaOH | |Mg |Silver Or Gray |Odorless |Forms a white powder |MgO+H2 |Mg(OH2)+H2 |Blue |MgCL2+H2 |MgOH+Na | |Cu | Orange |Odorless |Glows dull red |NO REACTION |Mg(OH2)+H2 |Blue |No Reaction |Cu(OH)2+Na | |Zn | Bluish-white |Odorless |Turns yellow |No Reaction |ZnO+H2 |Blue |ZnCL2+H2 |Na+Zn(OH)2 | |MgO | White |Odorless | |Mg(OH)2) |Mg(OH)2) |Blue |MgCL2+H2O |MgOH+NaO | |CuCO3 | Green |Odorless |Forms Copper Oxide & Carbon dioxide gas |CO2+Ca(OH) 2 |CO2+Ca(OH) 2 |Green |CuCl2+H2CO3 |CuOH+NaCO3 | |Cu(NO3)2 | Blue crystals |Slight | | |Cu2+NO3+H2O |Blue |CuCl2+2HNO3 |CuOh2+NaNO3 | |NaCl |White |Odorless |Melts & become clear liquid | |Na+Cl+H2O |No Color |No Reaction |NaCl+NaOH | | Conclusion: The purpose for this experiment was to combine different chemicals to see if a physical or a chemical change occurred. A physical change happens when the substance changes in appearance yet maintains its physical and chemical properties. A chemical change occurs when a different substance forms with newly formed physical and chemical properties. The first substance was magnesium. Before it was heated, it was a shiny silver strip.
4. Chlorine, Cl 2, is a strong oxidizing agent found in bleach. 10.0 cm3 of bleach solution was added to 25.0 cm3 of 0.4M Sn2+ solution acidified with sulphuric acid and made up to 100 cm3. 10.0 cm3 of the resulting solution containing the unreacted Sn2+ was titrated against 0.02M K2Cr2O7. Given that 11.40 cm3 of K2Cr2O7 was required for complete oxidation, a) Calculate the numbers of moles of Cr2O7- used.
With the development of the atomic theory, Oxidation ‘de-electronation’ could be defined as many, as the loss of electrons or the gain of oxygen, e.g., Oxidation of a potassium atom to a potassium ion K(S) → K(S)+ + e- and Oxidation of carbon to carbon dioxide (the more electronegative oxygen obtains greater share of carbon electrons) C(G) + O2(G) → CO2(G). While reduction ‘re elecronation’ could also be defined as the gain of electrons or the loss of oxygen, e.g., reduction of a chlorine atom to a chloride ion Cl(G) + e- → Cl(G)- and reduction of carbon dioxide to carbon monoxide CO2(G) + C(G) → 2CO(G). For these reactions to process, the presence of reactants that involve transferring electrons between reactants to form products should be available; these reactants are called reducing and oxidizing agents. An Oxidizing agent or oxidant, gains an electron, which is, reduced in a chemical reaction i.e. an electron acceptor; this means it decreases oxidation state by oxidizing other substances to gain electrons.