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All values refer to 25 °C and to the thermodynamically stable standard state at that temperature unless noted. Values from CRC refer to "100 kPa (1 bar or 0.987 standard atmospheres)".
Note that the especially high molar values, as for paraffin, gasoline, water and ammonia, result from calculating specific heats in terms of moles of molecules. If specific heat is expressed per mole of atoms for these substances, none of the constant-volume values exceed, to any large extent, the theoretical Dulong–Petit limit of 25 J⋅mol ...
Since 2019, a mole of any substance has been redefined in the SI as the amount of that substance containing an exactly defined number of particles, 6.022 140 76 × 10 23. The molar mass of a compound in g/mol thus is equal to the mass of this number of molecules of the compound in grams.
10.28 g/cm 3: WEL (near r.t.) 10280 kg/m 3: LNG (at r.t.) 10.28 g/cm 3: CRC (near r.t.) 10.2 g/cm 3: 43 Tc technetium (Tc-98 ?) use: 11 g/cm 3: WEL (near r.t.) 11500 kg/m 3: LNG (at r.t.) (Tc-98) 11 g/cm 3: CRC (near r.t.) 11 g/cm 3: 44 Ru ruthenium; use: 12.45 g/cm 3: WEL (near r.t.) 12370 kg/m 3: LNG (at 20 °C) (12.45 rel. to water at 4 °C ...
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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
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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 dividing the mass of copper by its molar mass: 63.55 g/mol.