Chemistry Notebook lab 2

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Chemistry Notebook Name: Kieria Brewer Date: 07/12/2023 Experiment #: 2 Title: Chemical Reactions Purpose: To study and observe 6 types of simple chemical reactions and reversible reactions. Procedure: Experiment 1: Test tube 1 contains HCl (colorless solution) while test tube 2 contains AgNO 3 (clear solution). The contents of test tube 1 are then poured into test tube 2. A white precipitate is formed that is identified as silver chloride (AgCl). A stopper is placed onto test tube 2 before the tube is inverted to mix any remaining HCl with any remaining AgNO 3 . Experiment 2: There are two new test tubes. Test tube 1 contains KI (colorless solution) and test tube contains Pb(NO 3 ) 2 (colorless solution). The contents of test tube one is then emptied into test tube two. A yellow precipitate is observed (PbI 2 ). A stopper is placed on top of test tube 2 and the tube is inverted. Experiment 3: There are two clean test tubes. Test tube 1 contains NaOH (colorless solution) and test tube 2 contains HCl (colorless solution). The temperature of each solution is taken. Both solutions had a temperature of 21.5 degrees Celsius. The contents of test tube one is then emptied into test tube 2. The solution is then poured back into the now empty test to help mix the two solutions. The temperature is then taken of the mixed solution, which read at 31.0 degrees Celsius. No precipitate is observed. Experiment 4: There are two test tubes with one containing HCL and the other containing NaHCO 3 . Both are colorless solutions. HCL is then added to the NaHCO 3 . Bubbles are formed within the mixed solution. This is CO 2 being released. Experiment 5: Barium Hydroxide is added to a clean unused beaker. Ammonium nitrate is then added into the same beaker. A small amount of water is mixed into the beaker. The contents of the beaker are then mixed with the temperature probe. The temperature decreases from a reading of 22 degrees C to -8 degrees C. Ammonia gas is detected by the use of a neutral litmus strip. The strip turns from a pinkish purple color to blue.

Chemistry Notebook Experiment 6: There is a test tube with concentrated HCl. Zinc metal is then added which causes bubbles to form as the hydrogen is being displaced as a gas. Experiment 7: Copper is added to a beaker containing silver nitrate (colorless solution). The beaker is stationed on top of a stirrer to keep the mixture agitated. The copper is then stirred around in the solution. The copper pieces begin to change to a grayish black color and the solution now has a blueish tint to it. The stirrer is then turned off to allow the silver particles to settle. Experiment 8: A match head swiped against the surface of the matchbox strike pad to create a spark. A flame is created. Experiment 9: A match is struck to create a flame. The flame is then placed against the wick of the candle. The candle wax undergoes combustion as it burns. Experiment 10: Hydrogen peroxide is added to an empty test tube. Manganese dioxide is then added to the test tube. The solution then begins to bubble as oxygen gas is given off. Experiment 11: Iodine is added to an empty beaker that is stationed on top of a stirrer. The stirrer is then turned on. Zinc is then added to same beaker using a scoopula. The mixture is left to react for 20 minutes. The solution is poured off and the water is boiled out of the mixture to leave a white substance in the beaker. Experiment 12: A piece of copper ribbon is placed into an open flame using a pair of tongs. The copper reacts with oxygen and begins to turn a dull black color. Experiment 13: A solution containing Methylene blue indicator is held in a flask with a stopper. The solution is then shaken which turns the sol0from colorless to blue. The solution is then left to sit while the sugars in the solution reduce the methylene blue back to its colorless state. This can be repeated until the sugars that are present have been depleted. Data/Results/Calculations: 1. Double Displacement Reaction Ag + NO 3 - + H + Cl - → H + NO 3 - + AgCl↓ Silver Nitrate Hydrochloric Acid Nitric Acid Silver Chloride Solution Solution Solution Precipitate  A white precipitate was formed by mixing the two colorless solutions. 2. Double Displacement Reaction Pb +2 (NO 3 - ) 2 + 2 K + I - → K + NO 3 - + PbI 2 ↓

Chemistry Notebook Lead Nitrate Potassium Iodide Potassium Nitrate Lead Iodide Solution Solution Solution Precipitate  A yellow precipitate was formed by mixing two colorless solutions, 3. Acid- base (Double Displacement) Reaction H + Cl - + Na + OH - → Na + Cl - + H 2 O + Heat Hydrogen Chloride Sodium Hydroxide Sodium Water Solution Solution Chloride  Two colorless solutions are mixed an no precipitate is formed. Heat and water are products. 4. Acid- base (Double Displacement) Reaction H + Cl - + Na + HCO 3 - → Na + Cl - + H 2 O + CO 2 + Heat Hydrogen Chloride Sodium Sodium Water Carbon Solution Bicarbonate Chloride Dioxide  Two colorless solutions are mixed and gas bubbles form. 5. Endothermic Reaction 2 NH 4 NO 3 + Ba(OH) 2 + Heat → Ba(NO 3 ) 2 + 2NH 3 ↑ + 2 H 2 O Ammonium Barium Barium Ammonia. Water Nitrate Hydroxide Nitrate Gas  Two colorless solids are mixed to form ammonia gas and water. 6. Single Displacement Reaction Zn + 2 H + 2 Cl - → Zn +2 2Cl - + H 2 ↑ + Heat Zinc Hydrogen Chloride Zinc Chloride Hydrogen Solution Solution Gas  A grey solid (zinc) is mixed with a colorless solution (hydrogen chloride) to produce a colorless solution (zinc chloride) and a colorless gas (hydrogen gas) 7. Single Displacement Reaction Cu + 2 Ag + 2 NO 3 - → Cu +2 2 NO 3 - + 2 Ag ↓ Copper Silver Nitrate Copper nitrate Silver Element Solution Solution  A reddish brown solid (copper) is mixed with a colorless solution (silver nitrate) to produce a blue colored solution (copper nitrate) and a gray solid (silver) 8. Combustion (burning) Reaction 2 KClO 3 ----------  2 KCl + 3O 2 ↑ S (sulfur) SO 3 + Heat ( Causes the wood of the match to burn) 9. Combustion (burning) Reaction C 25 H 52 + 38 O 2 → 25CO 2 ↑ + 26 H 2 O + Heat (+flame) Candle wax oxygen Carbon dioxide Water Air Gas  A colorless gas (candle wax) is mixed with a colorless gas (oxygen) to produce a colorless gas (carbon dioxide), water, and heat. 10.Decomposition Reaction 2H 2 O 2 -------  2H 2 O + O 2 ↑ Hydrogen peroxide MnO 2 Water Oxygen gas

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Chemistry Notebook  MnO 2 acts as the catalyst in this reaction 11.Synthesis Reaction Zn + I 2 → ZnI 2 Zinc Iodine Zinc iodide  A reddish brown solution (iodine) is mixed with a gray powder (Zinc) to produce a white solid (zinc iodide). 12.Synthesis Reaction 2Cu + O 2 → 2CuO Copper oxygen gas Copper oxide  A reddish brown solid (copper) is mixed with a colorless gas (oxygen) to produce a black solid (Copper oxide) 13.Reversible Reaction  A colorless solution reacts with oxygen to produce a blue colored solution. The sugars in the solution then reduce the solution to change it back to a colorless solution. Conclusions: It is known that a reaction occurs if there is a color change, change in temperature, gas is given off, a precipitate is formed or if water is present as a product. Not all reversible reactions are equilibrium reactions. Notes:  During a chemical reaction one of the following typically occurs. 1. Heat is given off (an exothermic reaction) 2. A precipitate (solid product) is formed. 3. A gas is given off. 4. Water ( H 2 O) is formed as a product 5. A color change is present  Double Displacement Reaction- A reaction in which the positive and negative ions of two reactants are interchanged.

Chemistry Notebook  Acid- base (double displacement) reaction- A reaction in which the positive and negative ions of acid and base reactants are interchanged with the evolution of heat and usually the formation of water.  Exothermic- Reaction where heat is given off.  Acid- a reactant containing a H + ion which can be donated  Base- a reactant whose anion ( - ion) can accept a H + ion  Endothermic – reaction where heat is absorbed  Single Displacement Reaction- A reaction in which a reactant element replaces the positive or negative ion of another reactant compound, yielding a new product element and compound.  Combustion - A reaction in which O 2 gas reacts with another compound to form one of more oxide products, accompanied by the generation of much heat ( and often a flame)  Decomposition Reaction- A reaction characterized by a greater number of product substances than the number of react substances  Catalyst- used to speed up a reaction without being consumed  Enzyme is a biochemical catalyst  Composition Reaction- A reaction characterized by a lesser number of product substances than the number of reactant substances  Reversible Reactions- equilibrium reactions are reversible with the forward reaction ( written left to right) converting reactants to products and the reverse reaction ( written right to left) converting those same products to the same reactants under similar conditions  Some reversible reactions are not equilibrium reactions

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