what is chemical mole
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Understanding the Mole Unit of Measurement Like all units, a mole has to be based on something reproducible. A mole is the quantity of anything that has the same number of particles found in 12.000 grams of carbon-12. That number of particles is Avogadro's Number, which is roughly 6.02x10 23. A mole of carbon atoms is 6.02x10 23 carbon atoms. A mole of chemistry teachers is 6.02x10 23 chemistry teachers. It's a lot easier to write the word 'mole' than to write '6.02x10 23 ' anytime you want to refer to a large number of things! Basically, that's why this particular unit was invented.
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How Much Water Is a Mole of Water? A mole is a unit of measuring the quantity of anything. A single mole is set to the number of particles found in 12.000 grams of carbon-12. This number is 6.022 x 1023 carbon atoms. The number 6.022 x 1023 is known as Avogadro's Number. A mole of carbon-12 atoms has 6.022 x 1023 carbon-12 atoms.
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- 1 A mole of any substance is 6.02×10 23 molecules of that substance. 2  You can use this as a conversion factor to turn moles into molecules. 3  For example, to figure out how many molecules there are in 0.001 moles of water,
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Mole Concept Visualizing a mole as a pile of particles, however, is just one way to understand this concept. A sample of a substance has a mass, volume (generally used with gases), and number of particles that is proportional to the chemical amount (measured in moles) of the sample.
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Mole-to-Mole Ratios and Calculations of a Chemical Equation Performing stoichiometry involves the use of a special chemical counting unit: the mole. Just to review for a moment, a mole isn't an animal. Well, it is, but not in chemistry. In chemistry, a mole is a unit of measurement, such that one mole of a substance contains 6.022 * 10^23 particles.
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Definition of Terms The Mole. The term mole literally means a small mass. It is used as the bridge between chemistry on the atomic and macroscopic scale. If the mass of a single 12 C atom is 12.000 amu, then one mole of these atoms would have a mass of 12.000 grams.
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- As of 2011, the mole is defined by BIPM to be the amount of substance of a system which contains the same number of elementary entities (e.g. atoms, molecules, ions, electrons) as atoms in 0.012 kilograms of carbon-12 (12 C), the isotope of carbon with relative atomic mass 12.he mole may also be used to express the number of atoms, ions, or other elementary entities in a given sample of any substance. The concentration of a solution is commonly expressed by its molarity, defined as the number of moles of the dissolved substance per litre of solution.
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Mole (unit) The mole is widely used in chemistry as a convenient way to express amounts of reactants and products of chemical reactions. For example, the chemical equation 2 H2 + O2 → 2 H2O implies that 2 moles of dihydrogen (H2) and 1 mole of dioxygen (O2) react to form 2 moles of water (H2O).
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The mole (mol) As a result of the definition, the mole contains a defined number of entities, usually atoms or molecules. This number is the Avogadro constant (NA). This number is a dauntingly large figure. This number of sand grains would cover the United Kingdom to a depth of about 40 centimetres.
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- 4 Chapter 3 7 The Mole •The mole (mol and abbreviated n) is a unit of measure that allows us to make comparisons between substances that have different masses• A mole is Avogadro’s number of atoms, that is 6.022 ×10 23 atoms.
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Chemical Formulas Key Terms Avogadro's number. the number of particles found in exactly one mole of any pure substance,6.022*10^23. chemical formula. a representation that shows the number of atoms of each kind of element in the chemical compound.
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SI base unit Definitions of the SI base units. 1. The mole is the amount of substance of a system which contains as many elementary entities as there are atoms in 0.012 kilogram of carbon 12; its symbol is mol..
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Amount of substance The mole is defined as the amount of substance that contains an equal number of elementary entities as there are atoms in 0.012kg of the isotope carbon-12. This number is called Avogadro's number and has the value 6.02214179(30)×1023.
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mol The amount of an element or substance that has a mass in grams numerically equal to the atomic or molecular weight of the substance. For example, carbon dioxide, CO2, has a molecular weight of 44; therefore, one mole of it weighs 44 grams. The number of atoms or molecules making up a mole is Avogadro's number.
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Chapter 3 Molecules and Atoms Chapter Review As of 2011, the mole is defined by BIPM to be the amount of substance of a system which contains the same number of elementary entities (e.g. atoms, molecules, ions, electrons) as atoms in 0.012 kilograms of carbon-12 (12 C), the isotope of carbon with relative atomic mass 12.
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mole Definition of mole. : the base unit of amount of pure substance in the International System of Units that contains the same number of elementary entities as there are atoms in exactly 12 grams of the isotope carbon 12.
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NPL's guide to the mole (mol) What is the mole? The mole is the SI base unit that measures amount of substance. The symbol for amount of substance is n. By definition, the mole contains a defined number of entities (usually atoms or molecules). This number is called 'the Avogadro constant' (N A). The mole is used to describe a practical quantity of material.
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Amount of Substance In short, the molar mass is the mass of one mole of any particular substance. In the SI units system a mole is defined by the amount of carbon atoms there are in 12g of carbon-12 (the nucleus of a carbon-12 atom contains 6 protons and 6 neutrons, hence carbon-12).
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General Chemistry/Print version Chemists often use a unit called the mole to measure quantities. A mole is defined as 6.022 x 10 to the 23rd atoms or molecules of a substance. When the substance is dissolved, the concentration or number of moles of substance per liter of solvent is called the molarity.
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- Avogadro's number. The number of atoms or molecules in a mole of a substance, approximately 6.0225 × 1023. It is based on the number of carbon atoms in 12 grams of carbon 12.
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Mole (unit) The number of moles of a sample is the sample mass divided by the molar mass of the material. History. The history of the mole is intertwined with that of molecular mass, atomic mass unit, Avogadro's number and related concepts.
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Molecular Weight Calculator Also, important in this field is Avogadro's number (NA) or Avogadro's constant (6.0221 x 1023). The term mole is defined in that one mole of a substance with a molecular (or atomic) mass of one (1), will have a mass of 1 gram. Or 1 mole of a substance will contain Avogadro's number of that substance.
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Molar Solution A molar solution is an aqueous solution that contains 1 mole (gram-molecular weight) of solute in 1 liter of the solution. This is the method most frequently used by chemists to express concentration. Molar concentration (molarity) is not same as molar solution. Molarity is the number of moles of solute per liter of solution.
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Amount of substance The SI unit for amount of substance is the mole. It has the unit symbol mol. The mole is defined as the amount of substance that contains an equal number of elementary entities as there are atoms in 12 g of the isotope carbon-12.This number is called Avogadro's number and has the value 7023602214085700000♠6.022140857(74)×1023.he mole is defined as the amount of substance that contains an equal number of elementary entities as there are atoms in 12 g of the isotope carbon-12.