EltaMD sunscreens help prevent sunburn and decrease the risk of skin cancer and early skin aging caused by the sun, when used with other sun protection measures. EltaMD sunscreens are formulated with transparent zinc oxide and are noncomedogenic, sensitivity-free, fragrance-free and paraben-free. FACIAL SUNSCREEN For specific skin types BODY & FACIAL SUNSCREEN For all skin types EltaMD broad-spectrum sunscreens provide safe, broad-spectrum ultraviolet (UV) protection. A broad-spectrum sunscreen helps prevent sunburn and if used as directed with other sun protection measures, decreases the risk of skin cancer and early skin aging caused by the sun. Ultraviolet, or UV rays, are part of the invisible energy that comes from the sun. UVA (aging) rays account for 95% of our sun exposure. They cause skin aging and contribute to skin cancer. UVA rays penetrate deeply into the skin layers, damaging collagen and cells which leads to wrinkling, hyperpigmentation and loss of elasticity. UVB (burning) rays mostly affect the outer layer of the skin. They cause sunburns and tanning that increase the risk of skin cancer and other disorders. The risk for skin cancer doubles in people who have had five or more sunburns. Skin Cancer Foundation (Nov. 2010) When wearing EltaMD sunscreens, the UVA and UVB rays reflect and scatter away from your skin, providing you protection from sunburn. EltaMD sunscreens help prevent sunburn and, if used as directed with other sun protection measures, decrease the risk of skin cancer and early skin aging caused by the sun. HOW EltaMD SUNSCREENS WORK All EltaMD sunscreens are formulated with zinc oxide, a natural, mineral compound. Because zinc maintains its protective ability in the sun, it is more photostable than some chemical ingredients that may degrade. Zinc sunscreen blocks the widest spectrum of UVA and UVB rays, protecting skin against burning and the premature appearance of aging and risk of skin cancer. Zinc is safe for even the most sensitive skin types.

Synthetic Iron Oxides have become increasingly important due to their pure hue, consistent properties, and tinting strength. Single-component forms are mainly produced with red, yellow, orange and black colours. Their composition corresponds to that of minerals hematite, goethite, lepidocrocite, and magnetite. Brown pigments usually consist of mixtures of red and/or yellow and/or black iron oxides. Its current use is mostly in construction, coatings, ceramics, paint, ink, rubber, plastics, cosmetics etc. The building materials industry is the biggest user of Iron Oxide Pigments. Uses include colouring concrete and mortar because of their good dispersability and good tinting strength. They are extensively used in the manufacture of Paving Blocks, Chequered Tiles, Designer Tiles, Stamped Concrete etc. Paints industry is the second largest user of Iron Oxide Pigments. Most paint applications require use if micronized and dispersible grades of pigments to get optimum colouring effects and maintain paint film strength. Pigments used in Plastics need high purity, tinting strength, high heat resistance and good dispersibility. Special applications include that in Ceramic Colours, Drugs, Cosmetics, Rubber, Brake Linings, Wood Polish, Cork Sheets, Fertilizers and Cattle Feed. New applications include catalysts in petroleum industry, in oil drilling rigs, in compound pigments, copy machine powder, and magnetic differentiate materials.

Calcium Hydroxide is a white powder or colourless crystal with a chemical formulation of Ca(OH)2. It is obtained when Calcium Oxide is mixed with water. Calcium Hydroxide has a number of synonyms including slaked lime, pickling lime, builder’s lime, hydrated lime. It is also known as slack lime or cal. You can purchase Calcium Hydroxide on Amazon. Uses of Calcium Hydroxide Calcium Hydroxide has a wide number of uses. For example, it is used in water treatment plants for treating sewage and it is also used to raise the pH of water where naturally occurring acidic water may damage pipe work. Calcium Hydroxide is widely used in the paper manufacturing industry, as a component in the Kraft process of manufacture. Calcium Hydroxide is a widely available and inexpensive substance and its uses range from whitewash and plaster, to petrochemicals, brake pads, pesticides and as an active ingredient in hair removal creams. Calcium Hydroxide is also widely used in food manufacture and preparation including the preparation of pickles and relishes, to process water for the soft drinks industry, in the sugar industry where it is used to separate sugar from sugar cane, to fortify fruit drinks and cordials, and as a Calcium supplement in baby milk. Native Americans have been using Calcium Hydroxide in cooking for hundreds of years, where it is known as ‘cal’. It is used to aid digestion, to increase absorption of certain substances and to enhance the effects of various naturally occurring stimulants enjoyed by Native American tribes people. Safety Hazards Calcium Hydroxide presents a number of safety hazards. It can cause irritation to the respirations tract resulting in coughing and shortness of breath. It is a gastric irritant and ingestion can cause severe pain, vomiting, diarrhoea and eventually collapse. Calcium Hydroxide is corrosive to skin and can cause severe burns and blistering. Calcium Hydroxide is corrosive to the eyes, causing severe pain and irritation, with the possible result of causing blindness. Prolonged skin exposure can produce severe irritation and dermatitis. Persons with pre-existing skin conditions or respiratory conditions are especially susceptible to the effects of Calcium Hydroxide.

Epsom salts, or magnesium sulfate, is becoming an increasingly common supplement for horses. Magnesium plays an important part in nerve and muscle function, and horses deficient in this important element can show signs of nervousness, wariness, excitability, and muscle tremors. This gives magnesium its reputation for having a calming influence on equines. A deficient horse is likely to have a poor tolerance to work and its muscles will tie up quite quickly. Magnesium is also known to play an important part in reducing equine obesity, and can lessen the risk of laminitis in animals prone to it during periods of strong spring grass growth. But like most things, you can easily end up giving your horse too much. Epsom salts is cheap and there is a danger that horse owners may be providing too much in their horse’s diet. Epsom salts is best known as a laxative. Give your horse an overly generous amount and, just like people, they’ll be feeling the effects of diarrhoea. Anything greater than one level tablespoon a day per 100kg of your horse’s bodyweight is likely to result in a case of the runs. Supplementation rates: • 31 mg/kg/day of MgO or • 64 mg/kg/day of MgCO3 or • 93 mg/kg/day of MgSO4 While at the correct rate, it is an acceptable source of magnesium, you will probably be better feeding magnesium oxide or – the Rolls-Royce of magnesium supplements – magnesium aspartate. Excessive magnesium will be excreted in the urine, but major overdoses have been linked to heart conduction problems and renal trouble, so it’s important you don’t overdo it. A study looking at magnesium uptake in horses was conducted by six veterinarians at the Department of Veterinary Biosciences, College of Veterinary Medicine, at Ohio State University. The magnesium requirement of a typical horse was put at 13 milligrams per kilogram of bodyweight per day. Horses that are growing, lactating, or in work will use more each day. For example, a lot of magnesium can be lost in sweat. For such animals, the quantity could be increased 1.5 to 2 times the maintenance dose. Opinion appears to vary on whether magnesium supplementation is needed at all. It will, of course, depend in part on whether the soils on which a horse is grazing are deficient in the element. Any such deficiency will be reflected in the grass grown. In general, a horse is likely to get between 60 per cent and 100 per cent of its daily magnesium needs through a normal forage diet. Deficiencies are most likely in spring, during periods of strong grass growth, and even in winter on pastures in milder areas where grass is being pushed along with fertiliser. Grass in both circumstances is likely to be low in magnesium, sodium, and soluble carbohydrates, and most likely high in nitrogen and potassium. This is a double whammy, as high potassium levels can slow the absorption of what little magnesium there is, while sodium (which is low in these situations) is known to help its uptake. Mechanisms affecting magnesium uptake in a horse are complex, and not always related to too little magnesium in the diet. It is just as likely that magnesium deficiency is caused by too much potassium in the diet inhibiting uptake. Potassium is not the only potential player in this complex equation. The presence and proportions of calcium, phosphorous, and fats in the diet can also play a part in the ability of a horse to use the magnesium in its diet.

Oxidation-reduction reactions (redox reactions) are reactions in which electrons are lost by an atom or ion in one reactant and gained by an atom or ion in another reactant. Although electrons are gained and lost in these reactions, the balanced equation for a redox reaction does not show the electrons that are being transferred. In order to tell whether a redox reaction has occurred or not, we need a way to keep track of electrons. The best way to do so is by assigning oxidation numbers to the atoms or ions involved in a chemical reaction. Oxidation numbers are hypothetical numbers assigned to an individual atom or ion present in a substance using a set of rules. Oxidation numbers (or oxidation states as they are also called) can be positive, negative, or zero. It is VERY IMPORTANT to remember that oxidation numbers are always reported for one individual atom or ion and not for groups of atoms or ions . The following rules are used to assign oxidation numbers. Chem 1115 students will have these rules available on exams. Chem 1215 students must memorize these rules. Oxidation Number Rules The oxidation number for an atom in its elemental form is always zero. A substance is elemental if both of the following are true: only one kind of atom is present charge = 0 Examples: S8: The oxidation number of S = 0 Fe: The oxidation number of Fe = 0 The oxidation number of a monoatomic ion = charge of the monatomic ion. Examples: Oxidation number of S2- is -2. Oxidation number of Al3+ is +3. The oxidation number of all Group 1A metals = +1 (unless elemental). The oxidation number of all Group 2A metals = +2 (unless...

Molar mass of Fe3O4 = 231.5326 g/mol Molecular weight calculation: 55.845*3 + 15.9994*4 Element Symbol Atomic Mass # of Atoms Mass Percent Fe 55.845 72.359% 15.9994 27.641% In chemistry, the formula weight is a quantity computed by multiplying the atomic weight (in atomic mass units) of each element in a chemical formula by the number of atoms of that element present in the formula, then adding all of these products together. Finding molar mass starts with units of grams per mole (g/mol). When calculating molecular weight of a chemical compound, it tells us how many grams are in one mole of that substance. The formula weight is simply the weight in atomic mass units of all the atoms in a given formula. If the formula used in calculating molar mass is the molecular formula, the formula weight computed is the molecular weight. The percentage by weight of any atom or group of atoms in a compound can be computed by dividing the total weight of the atom (or group of atoms) in the formula by the formula weight and multiplying by 100. A common request on this site is to convert grams to moles. To complete this calculation, you have to know what substance you are trying to convert. The reason is that the molar mass of the substance affects the conversion. This site explains how to find molar mass. Formula weights are especially useful in determining the relative weights of reagents and products in a chemical reaction. These relative weights computed from the chemical equation are sometimes called equation weights. Using the chemical formula of the compound and the periodic table of elements, we can add up the atomic weights and calculate molecular weight of the substance. The atomic weights used on this site come from NIST, the National Institute of Standards and Technology. We use the most common isotopes. This is how to calculate molar mass (average molecular weight), which is based on isotropically weighted averages. This is not the same as molecular mass, which is the mass of a single molecule of well-defined isotopes. For bulk stoichiometric calculations, we are usually determining molar mass, which may also be called standard atomic weight or average atomic mass.

How many moles Calcium Oxide in 1 grams? The answer is 0.004. We assume you are converting between moles Calcium Oxide and gram . You can view more details on each measurement unit: molecular weight of Calcium Oxide or grams The molecular formula for Calcium Oxide is CaO. The SI base unit for amount of substance is the mole. 1 mole is equal to 1 moles Calcium Oxide, or 56.0774 grams. Note that rounding errors may occur, so always check the results. Use this page to learn how to convert between moles Calcium Oxide and gram. Type in your own numbers in the form to convert the units! In chemistry, the formula weight is a quantity computed by multiplying the atomic weight (in atomic mass units) of each element in a chemical formula by the number of atoms of that element present in the formula, then adding all of these products together. Finding molar mass starts with units of grams per mole (g/mol). When calculating molecular weight of a chemical compound, it tells us how many grams are in one mole of that substance. The formula weight is simply the weight in atomic mass units of all the atoms in a given formula. If the formula used in calculating molar mass is the molecular formula, the formula weight computed is the molecular weight. The percentage by weight of any atom or group of atoms in a compound can be computed by dividing the total weight of the atom (or group of atoms) in the formula by the formula weight and multiplying by 100. A common request on this site is to convert grams to moles. To complete this calculation, you have to know what substance you are trying to convert. The reason is that the molar mass of the substance affects the conversion. This site explains how to find molar mass. Using the chemical formula of the compound and the periodic table of elements, we can add up the atomic weights and calculate molecular weight of the substance.

Magnesium oxide comes as a tablet and capsule to take by mouth. It usually is taken one to four times daily depending on which brand is used and what condition you have. Follow the directions on the package or on your prescription label carefully, and ask your doctor or pharmacist to explain any part you do not understand. Take magnesium oxide exactly as directed. Do not take more or less of it or take it more often than prescribed by your doctor. Take any other medicine and magnesium oxide at least 2 hours apart. If you are using magnesium oxide as a laxative, take it with a full glass (8 ounces [240 milliliters]) of cold water or fruit juice. Do not take a dose late in the day on an empty stomach.

Electrochemical tests, including anodic polarization, Tafel polarization and electrochemical impedance spectrum (EIS), were used to evaluate the anodic behaviors of a ternary alloy of Ni0.94Si0.04Al0.02 in molten NaOH at 773 K. The results revealed that a conductive passivation layer had formed during electrolysis, which protected the Ni0.94Si0.04Al0.02 substrate from further attacked. An in situ test of anodic gases using a mass spectra indicated that oxygen was emitted from the interface of the Ni0.94Si0.04Al0.02 anode. Meanwhile, the iron sponge can be electrochemically produced when Fe2O3 is used as cathode. The significant result is that the Ni0.94Si0.04Al0.02 alloy is promising as an inert anode in molten NaOH electrolyte for a green metallurgical process. Keywords Inert anode; Molten salts; Oxygen; Iron

Oxidations Of Alcohols With “Eye Of Newt”, “Wing of Bat”, and “Powdered Unicorn Horn” Here we are, at least fifteen articles into this series on alcohols, and all we’ve really talked about is substitution and elimination reactions, with a little bit of acid-base chemistry mixed in. We haven’t even scratched the surface of one of the most important classes of reaction for alcohols – one that becomes crucial as you move into Org 2. I’m talking about oxidation reactions. What do I mean by an “oxidation reaction”, anyway? Let’s start by examining the bonds that form and the bonds that break in this process, where we convert a primary alcohol to an aldehyde: [ No, “Eye of newt” doesn’t actually do oxidation reactions: I’m being a bit coy with exact reagents for now, because as I’ll explain in a bit, there are so many different reagents for oxidation of alcohols that many students get spooked by the fact that they look unfamiliar and fail to actually pay attention to the important part: the bonds that form and break in the reaction ! ] The key process here is that we’re forming a C-O bond and breaking a C-H bond on the same carbon. That’s a sure sign of an oxidation reaction. For more background on oxidation reactions in organic chemistry, check out this when I learned organic chemistry. The reagents that were given to us might have well been “eye of newt” and “powdered unicorn horn” since they were introduced without any background or context and disappeared just as quickly after the section on oxidation was over. It was only later that I understood that oxidation is not nearly as complicated as these weird reagents make it seem. In fact, the underlying process is in most cases extremely familiar – it’s just not taught that way! In the next post, we’ll discuss the common – and very familiar! – mechanistic step that (almost) all oxidation reactions you’ll learn have in common. Not only will oxidation reactions then become less mysterious. Note: it’s an oversimplification because the first step in oxidation of an aldehyde is generally addition of water to form a hydrate, which is then oxidized to the carboxylic acid. Some oxidants we call “weak” (e.g. CrO3, pyridine) can thus be “strong” if water is present. It’s a teaching kludge, but good enough for our purposes, for now.