Steel and Corrosion

It is a chemical reaction where the colors of both solution and iron strip changed. It is

Of all the out-of-state businessmen who invested in Minnesota’s iron mines, Henry W. Oliver was the most influential. Oliver was rich, but he wasn't rich enough to pay

Eleven mystery test tubes labeled from K-1 to K-11 contained: 6M H2SO4, 6M NH3, 6M HCl, 6M NaOH, 1M NaCl, 1M Fe(NO3)3, 1M NiSO4, 1M AgNO3, 1M KSCN, 1M Ba(NO3)2, 1M Cu(NO3)2 respectively. The contents of the test tubes were determined by chemical experiments. Solution K-1 contained NiSO4 because when solution K-9, ammonia which was identified by its pungent odor, was added, an inky dark blue color was made. Iron (Fe (NO3)3) was determined to be in test tube K-2. KSCN was found in test tube K-11 since Fe (NO3)3 and KSCN makes a bloody color when mixed together. Flame tests were conducted in which K-8

b) Iron and Barium were present in unknown 3. Assigned unknown reacted with all 4 reactants and formed precipitate with 3 of them (Sodium carbonate, sodium hydroxide and Sulfuric acid). During the experiment it reacted very similarly to Iron (III) nitrate and Barium nitrate. For example, with it was tested against Ammonium Chloride, the color of the solution changed to a light green, very identically to Iron (III) nitrate and Ammonium Chloride. Besides, unknown 3 formed an orange brownish precipitate when it was tested with sodium carbonate. Iron (III) nitrate acted similarly. Moreover, unknown 3 reacted similar to Barium nitrate when it was tested against ammonium chloride and sulfuric acid. It did not form any precipitate with ammonium chloride but formed a very light white precipitate, which is identical to barium nitrate’s reaction against sulfuric acid. Therefore, the two present metal in unknown 3 are Iron and barium.

The British also sent men who were capable of producing charcoal from wood. Charcoal was the main source of fuel used in the iron smelters. Charcoal was used to melt iron ores. The main area where the iron smelters were used was in the Chesapeake region. In the New South Alabama was the center of the iron industry as well as the steel industry.

The swift expansion of the industrial city, leads to numerous infrastructure problems, particularly in the sanitization and water supply sector. Their response to the rapidly increasing population was to utilize their industrial and mining capabilities as a easy solution. Cast iron pipes were mass produced then placed in the ground, solving the water and sanitization issue, so they thought. Cast iron is a sturdy, cheap, and easy made metal; because of its relatively simple process to produce, cast iron will corrode and perforate within seventy-five years of it being laid into the ground.

Back in the day they used anything that could make the metal rust but controlled the time and exposure to make sure that it didn’t completely rust through, so like an already mentioned took too much time and constant attention. Some of the substances that have been used in the past to speed the process up were blood, urine, and table salt.

The first reaction involves pyrite rock reacting with oxygen (air) and water to produce dissolved ferrous iron, sulfate, and acidity. The second reaction oxidizes the dissolved ferrous iron in acidic conditions and produces ferric iron and water. The third reaction involves the hydrolysis of the ferric iron to form ferric hydroxide and more acid. The ferric hydroxide is the orangey-red colored solid you see in the water (Juniata College).

Made with top-quality 22-gauge hot-dipped galvanized inner and outer steel that resists abrasion and provides superior durability, as

The experiment in this activity involves the reaction between a copper (II) chloride solution with iron nails and the mole ratios involved in the reaction. Measurements are taken to determine the moles of each reactant involved in the reaction and thus the number of atoms or molecules involved.

In this short paper I will cover my thoughts on the article provided for this week’s article summary, “Slow Rust Bluing: Science or Alchemy, American Gunsmith March 2009, by Dan Herman.” It’s not all that often that I’m eager to read one of these articles we’re given for article summaries. The bluing process interests me immensely, and I can’t wait to get to a point where I can re-blue a firearm to see how badly I do on my first job…lol.

Chloride Equation: Ag+ (aq) + Cl- AgCl (s) Sliver Nitrate- Adding dilute nitric acid. (Sliver nitrate + dilute nitric acid.)

This scientific report is about how much mass is lost in metals after being placed in 1 molar hydrochloric acid for 30 minutes. Tin, iron and zinc will be weighed and placed into test tubes which will then be filled with 1 molar hydrochloric acid. After 30 minutes the metals will be taken out and weighed again. It is expected that the more reaction that occurs, the more mass is lost. Tin is a metal and has many uses and is commonly used to coat other metals to prevent them from corroding. An example of this is in tin cans made of tin-coated steel. Iron is another common metal which rusts easily but it is very important as it is used to manufacture steel. Zinc is a metal which is most commonly used to galvanise metals

The purpose of this project was to discover how the pH level affects corrosion rate. The hypothesis was if the pH level affects the corrosion rate, then the lower the pH level is quicker the corrosion rate would be. This will happen because liquids below the pH level of 7 possess stronger acidic attributes. The effect of pH level on corrosion rate was determined by depositing a copper penny in each of three plastic cups, and then three different liquids by their pH levels, were assigned to be displaced into each cup formulating a chemical reaction to be observed. The results collected during this investigation contradicted with the intended result, this experiment was conducted to determine corrosion rate; Dana Puti Vingear (pH level: 4.5)

through the duration of the entire experiment. Part 1 involves the synthesis of an iron (III) oxalate complex. The iron is first presented in its Fe2+ form, so it must first be oxidized to