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Copper(II) nitrate describes any member of the family of inorganic compounds with the formula Cu(NO 3) 2 (H 2 O) x. The hydrates are hygroscopic blue solids. Anhydrous copper nitrate forms blue-green crystals and sublimes in a vacuum at 150-200 °C. [5] [6] Common hydrates are the hemipentahydrate and trihydrate.
In chemistry, the molar mass (M) (sometimes called molecular weight or formula weight, but see related quantities for usage) of a chemical compound is defined as the ratio between the mass and the amount of substance (measured in moles) of any sample of the compound. [1] The molar mass is a bulk, not molecular, property of a substance.
Many other oxyanions form complexes; these include copper(II) acetate, copper(II) nitrate, and copper(II) carbonate. Copper(II) sulfate forms a blue crystalline pentahydrate, the most familiar copper compound in the laboratory. It is used in a fungicide called the Bordeaux mixture. [65] Ball-and-stick model of the complex [Cu(NH 3) 4 (H 2 O) 2 ...
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 ...
Substance Formula 0 °C 10 °C 20 °C 30 °C 40 °C 50 °C 60 °C 70 °C 80 °C 90 °C 100 °C Barium acetate: Ba(C 2 H 3 O 2) 2: 58.8: 62: 72: 75: 78.5: 77: 75
Copper(II) chromite: Cu 2 Cr 2 O 5: Chromite (chromic acid) Copper(II) gluconate: C 12 H 22 CuO 14: Gluconate (gluconic acid) Copper(II) peroxide: CuO 2: Peroxide (hydrogen peroxide) Copper(II) usnate: C 18 H 14 CuO 7: Usnate Copper(II) oxychloride: Cu 2 (OH) 3 Cl: Hydroxide and chloride: Copper(II) naproxen: C 28 H 26 CuO 6: naproxen: Copper ...
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.
Equivalent weights may be calculated from molar masses if the chemistry of the substance is well known: sulfuric acid has a molar mass of 98.078(5) g mol −1, and supplies two moles of hydrogen ions per mole of sulfuric acid, so its equivalent weight is 98.078(5) g mol −1 /2 eq mol −1 = 49.039(3) g eq −1.