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.

Molar mass of Fe2O3 = 159.6882 g/mol Molecular weight calculation: 55.845*2 + 15.9994*3 Element Symbol Atomic Mass # of Atoms Mass Percent Fe 55.845 69.943% 15.9994 30.057% 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. 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. 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. 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. 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.

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Aluminum (aluminium) is the number one most abundant metal found in the Earth’s crust. With that being said, it’s no wonder that with our propensity for exploiting everything we can get our hands on, you will find something made from this metal in pretty much every home you see. I don’t mean to be an ass about it. I’m every bit as guilty as anyone else. Aluminum is cheap, it’s lightweight, and when it’s clean, it’s pretty nice to look at. You know, all shiny and silvery and stuff. Aluminum by itself isn’t all that useful. It’s too soft. Under most circumstances it is mixed with other metals like copper, zinc, magnesium, or manganese to create an alloy with greater strength and durability. Even with other metals thrown in there, aluminum alloys are still quite malleable and can be used for an absolutely ridiculous number of things. You will find aluminum used for cans (of course), pots and pans, utensils, siding, boats, machinery, wheels, motors, gutters, blinds, electrical work, paints, and the list goes on and on and on. It makes good sense, along with being cheap, abundant, and easy to work with, the stuff is also very resistant to corrosion. This is due to aluminum’s affinity for oxygen. You know that dull gray that’s been taking over your nice new aluminum pot? That’s what I’m talking about. That’s aluminum oxide, and that’s what we’re here to get rid of today. Yes, it protects your aluminum from corrosion. But as soon as you clean it off, it starts coming back again. Your aluminum is still protected, and now, because that layer of aluminum oxide isn’t nearly as thick as it was, your pan still looks nice. The method for cleaning aluminum found in this article is intended for unfinished aluminum like (but not limited to) that found in aluminum pots, pans, plates, cups, and utensils.