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The molecular formula C 6 H 8 O 6 (molar mass: 176.124 g/mol) may be: Ascorbic acid (vitamin C) Erythorbic acid; Glucuronolactone; Propane-1,2,3-tricarboxylic acid;
Atomic number Element Molar mass Formal standard atomic weight s.a.w., formal short Note Z calculated; g·mol −1 A r, standard [2] A r, abridged and conventional [2]; C 9 H 8 O 4: 180.159 g·mol −1
C 6 H 6 O 6 • − + L• + H 2 O + H + → C 6 H 8 O 7 + LH 2 C 6 H 6 O 6 • − + H 2 O + H + → C 6 H 8 O 7 + C 6 H 7 O − 6. Aqueous solutions of dehydroascorbate are unstable, undergoing hydrolysis with a half-life of 5–15 minutes at 37 °C (99 °F). Decomposition products include diketogulonic acid, xylonic acid, threonic acid and ...
Molecular weight (M.W.) (for molecular compounds) and formula weight (F.W.) (for non-molecular compounds), are older terms for what is now more correctly called the relative molar mass (M r). [8] This is a dimensionless quantity (i.e., a pure number, without units) equal to the molar mass divided by the molar mass constant .
The derived quantity relative molecular mass is the unitless ratio of the mass of a molecule to the atomic mass constant (which is equal to one dalton). [2] The molecular mass and relative molecular mass are distinct from but related to the molar mass.
where the pressure, p, is the atmospheric pressure, V is the measured volume of the vessel, T is the absolute temperature of the hot bath, and R is the gas constant. The molecular weight of the chemical is then simply the mass in grams of the vapor within the vessel divided by the calculated number of mole.
In solutions, mass concentration is commonly encountered as the ratio of mass/[volume solution], or m/v. In water solutions containing relatively small quantities of dissolved solute (as in biology), such figures may be "percentivized" by multiplying by 100 a ratio of grams solute per mL solution. The result is given as "mass/volume percentage".
The ideal gas equation can be rearranged to give an expression for the molar volume of an ideal gas: = = Hence, for a given temperature and pressure, the molar volume is the same for all ideal gases and is based on the gas constant: R = 8.314 462 618 153 24 m 3 ⋅Pa⋅K −1 ⋅mol −1, or about 8.205 736 608 095 96 × 10 −5 m 3 ⋅atm⋅K ...