HYPOTHESIS: Once I pour the baking soda solution on the silver it will remove the tarnish from the silver because aluminum is a more active metal than silver causing the silver sulfide to bond to the aluminum.
PURPOSE: The purpose of this experiment is to observe an oxidation-reduction reaction.
RAW MATERIALS:
aluminum foil
silver tarnished object- ring
Teflon frying pan
Pot to boil 1 quart of water
baking soda
container to measure out 1 quart of water
a tablespoon measure
wooden spoon
pennies
tap water-(source Ogallala Aquifer, treated by the City of Dalhart water department)
tweezers
SAFETY CONSIDERATIONS: Always think about safety first. Keep a rag close by for any water spills. Be extremely careful as you are dealing with HOT water. Keep something (tweezers) close by to handle silver object as the hot water will heat the silver. Remain in a ventilated room in case any odors are produced. Wear goggles or eye protective glasses.
EXPERIMENTAL PROCEDURE:
1. Ventilate the room.
2. Make a baking soda solution by
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I could not make out the odor as I did not want to keep sniffing in case it was unsafe to continuously smell. In addition, I noticed the process worked faster as I moved the ring against the aluminum with my wooden spoon. Because my ring was covered in a lot of tarnish I allowed it to sit in the solution for about 7 minutes and once the bubbles/fizz was barely noticeable, I took the ring out with my tweezers. Before the baking soda solution cooled, I place two pennies in the solution and observed nothing. I would like to include that I tried other jewelry (apparently they were not true silver) and nothing happened. I also tried to find quarters that were tarnished and learned they are only silver if they were made before 1965 (I use a debit card so I did not have very much change lying
2-ethyl-1,3-hexanediol. The molecular weight of this compound is 146.2g/mol. It is converted into 2-ethyl-1-hydroxyhexan-3-one. This compounds molecular weight is 144.2g/mol. This gives a theoretical yield of .63 grams. My actual yield was .42 grams. Therefore, my percent yield was 67%. This was one of my highest yields yet. I felt that this was a good yield because part of this experiment is an equilibrium reaction. Hypochlorite must be used in excess to push the reaction to the right. Also, there were better ways to do this experiment where higher yields could have been produced. For example PCC could have been used. However, because of its toxic properties, its use is restricted. The purpose of this experiment was to determine which of the 3 compounds was formed from the starting material. The third compound was the oxidation of both alcohols. This could not have been my product because of the results of my IR. I had a broad large absorption is the range of 3200 to 3500 wavenumbers. This indicates the presence of an alcohol. If my compound had been fully oxidized then there would be no such alcohol present. Also, because of my IR, I know that my compound was one of the other 2 compounds because of the strong sharp absorption at 1705 wavenumbers. This indicates the presence of a carbonyl. Also, my 2,4-DNP test was positive. Therefore I had to prove which of the two compounds my final product was. The first was the oxidation of the primary alcohol, forming an aldehyde and a secondary alcohol. This could not have been my product because the Tollen’s test. My test was negative indicating no such aldehyde. Also, the textbook states that aldehydes show 2 characteristic absorption’s in the range of 2720-2820 wavenumbers. No such absorption’s were present in my sample. Therefore my final product was the oxidation of the secondary alcohol. My final product had a primary alcohol and a secondary ketone
Any of a class of organic compounds that are fatty acids or their derivatives and are insoluble in water but soluble in organic solvents. They include many natural oils, waxes, and steroids.
Hand washing is very important in order to prevent infection (Leifso, Sheehan, & Knoll, Module 3, 2012). Routine hand washing involves turning on the water, applying soap and then washing for up to 20 seconds (CDC, 2009). All areas should be washed, including the front of the hands, back of the hands, in between fingers, and around the nails (CDC, 2009). After rinsing, paper towels are then used to dry the hands and close the tap (CDC, 2009). Alcohol based hand sanitizers should only be used if it is not possible to get to a sink and if the hands are not visibly dirty (Leifso, Sheehan, & Knoll, Module 3, 2012).
Purpose/Introduction: In this experiment, four elimination reactions were compared and contrasted under acidic (H2SO4) and basic (KOC(CO3)3) conditions. Acid-catalyzed dehydration was done on 2-butanol and 1-butanol; a 2o and 1o alcohol, respectively. The base-induced dehydrobromination was performed on 2-bromobutane and 1-bromobutane isomeric halides. The stereochemistry and regiochemistry of the four reactions were analyzed by gas chromatography (GC) to determine product distribution (assuming that the amount of each product in the gas mixture is proportional to the area under its complementary GC peak).
made from a form of aluminum soap mixed with the acid (Time, 2000). The formula was said to have
Aluminum is a lightweight, silvery metal. The atomic weight of aluminum is 26.9815; the element melts at 660° C (1220° F), boils at 2467° C (4473° F), and has a specific gravity of 2.7. Aluminum is a strongly electropositive metal and extremely reactive. In contact with air, aluminum rapidly becomes covered with a tough, transparent layer of aluminum oxide that resists further corrosive action. For this reason, materials made of aluminum do not tarnish or rust. The metal reduces many other metallic compounds to their base metals. For example, when thermite (a mixture of powdered iron oxide and aluminum) is heated, the aluminum rapidly removes the oxygen from the iron; the heat of the reaction is sufficient to melt the iron. This phenomenon is used in the thermite process for welding iron .
Greta Christina eloquently puts into words something I know in theory, but can be hard to understand in practice in heterosexual relationships. In Are we having sex now or what? Christina details her record keeping of how many people she had sex with, and what she counted as sex. She talks about the limiting misconception of sex only being coitus, and other acts not “counting.” Christina writes of how when she started having sex with women her outdated system of what was sex and what was not sex was completely destroyed. By limiting sex to “penis in vagina,” Christina was discounting some of her favorite sexual experiances, and including ones she did not particularly enjoy.
Gold bears quite a number of chemical properties that I will discuss in details down here. These point out on how gold behaves at various conditions. The chemical formula of gold is Au which is derived from its chemical name. When it comes to gold’s activity, it is not chemically active. This means that it greatly resists any kind of chemical reaction. In most cases, it rarely reacts with other chemicals. Gold is easily reduced from a compound to become a metal. It has two main compounds. These compounds are the Chloral-auric acid as well as the auric chloride. When we come to how gold reacts with certain acids, it is clear that there is an acid that is very able to dissolve this element. This acid is known as Aqua regia and is a combination of hydrochloric and nitric acids. Gold is not able to react with non-metals. Under this case, it only reacts with halogens and forms what is known as halides. The main alloys that can be used to make gold harder include platinum metal and silver (Tocci,
isn’t an ornate silver tea set that requires careful polishing, it probably needs to be
Alloys in the ornament manufacturing are a general use of gold. Because of it is...
treatment 2: blend cool water and apple cider vinegar in same quantities. Later rub down onto your affected elements with the answer. strive repeating a few times every day for numerous days.
Investigating the Effect of the Enzyme Catalyse On Hydrogen Peroxide Introduction The aim of this experiment is to determine the effects of varying enzyme (catalyse) on Hydrogen Peroxide. Hydrogen Peroxide + Catalyse à Water + Oxygen 2H2O2 à H2O + O2 + Heat Apparatus & Diagram [IMAGE][IMAGE][IMAGE][IMAGE][IMAGE][IMAGE][IMAGE] Bung Potato Hydrogen Peroxide Water Collected Oxygen Delivery Tube Measuring Cylinder [IMAGE] Using the Equipment Safely It is important that we use the apparatus carefully, as safety will be an issue throughout the whole experiment. We will wear goggles and an apron or lab coat to protect our eyes and clothes. As we are using enzymes and Hydrogen Peroxide we need to be extra careful, ensuring they don't come into contact with our eyes, skin or clothes. Catalyse is an enzyme found in all living cells.
In its pure form silver is a white, soft metal. Silver is extremely soft so a small amount of another metal is usually added to increase its hardness and strength. A metal silver is usually mixed with is copper. The element silver reflects 95 percent of light that strikes it, which makes it the most shiny of all the metals on the periodic table. The metal is located on the D
Back then, it was said silver was commonly used is Anatolia which is now modern Turkey. No one actually knows who discovered silver due to how incredibly far back it dates. Silver's symbol is Ag which comes from the Latin word Argentum. Silver is a transition metal. Due to it’s metal-like properties, it is located in group 11 and period 5.