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The mole ratio is also called amount ratio. [2] If n i is much smaller than n tot (which is the case for atmospheric trace constituents), the mole ratio is almost identical to the mole fraction . Mass ratio
Historically, the mole was defined as the amount of substance in 12 grams of the carbon-12 isotope.As a consequence, the mass of one mole of a chemical compound, in grams, is numerically equal (for all practical purposes) to the mass of one molecule or formula unit of the compound, in daltons, and the molar mass of an isotope in grams per mole is approximately equal to the mass number ...
Thus, for example, the average mass of a molecule of water is about 18.0153 daltons, and the molar mass of water is about 18.0153 g/mol. For chemical elements without isolated molecules, such as carbon and metals, the molar mass is computed dividing by the number of moles of atoms instead.
Mass to moles: Convert grams of Cu to moles of Cu; Mole ratio: Convert moles of Cu to moles of Ag produced; Mole to mass: Convert moles of Ag to grams of Ag produced; The complete balanced equation would be: Cu + 2 AgNO 3 → Cu(NO 3) 2 + 2 Ag. For the mass to mole step, the mass of copper (16.00 g) would be converted to moles of copper by ...
For example, water has a molar mass of 18.0153(3) g/mol, but individual water molecules have molecular masses which range between 18.010 564 6863(15) Da (1 H 2 16 O) and 22.027 7364(9) Da (2 H 2 18 O). Atomic and molecular masses are usually reported in daltons, which is defined in terms of the mass of the isotope 12 C (carbon-12).
The mole and the atomic mass unit (dalton) were originally defined in the International System of Units (SI) in such a way that the constant was exactly 1 g/mol, which made the numerical value of the molar mass of a substance, in grams per mole, equal to the average mass of its constituent particles (atoms, molecules, or formula units) relative ...
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Normality can be used for acid-base titrations. For example, sulfuric acid (H 2 SO 4) is a diprotic acid. Since only 0.5 mol of H 2 SO 4 are needed to neutralize 1 mol of OH −, the equivalence factor is: f eq (H 2 SO 4) = 0.5. If the concentration of a sulfuric acid solution is c(H 2 SO 4) = 1 mol/L, then its normality is 2 N. It can also be ...