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0.17308 g/cm 3 (from 23.1256 cm 3 /mole; at local min. density, from hcp melt at 0.699 K, 24.993 atm) 0.17443 g/cm 3 (from 22.947 cm 3 /mole; He-II at triple point hcp−bcc−He-II: 1.463 K, 26.036 atm) 0.1807 g/cm 3 (from 22.150 cm 3 /mole; He-I at triple point hcp−bcc−He-I: 1.772 K, 30.016 atm) 3 Li lithium; use: 0.512 g/cm 3: CR2 (at m ...
Chromium compounds are compounds containing the element chromium (Cr). Chromium is a member of group 6 of the transition metals. The +3 and +6 states occur most commonly within chromium compounds, followed by +2; charges of +1, +4 and +5 for chromium are rare, but do nevertheless occasionally exist. [3] [4]
For example, 50 g of zinc will react with oxygen to produce 62.24 g of zinc oxide, implying that the zinc has reacted with 12.24 g of oxygen (from the Law of conservation of mass): the equivalent weight of zinc is the mass which will react with eight grams of oxygen, hence 50 g × 8 g/12.24 g = 32.7 g.
The anhydrous form of chromium(II) acetate, and also related chromium(II) carboxylates, can be prepared from chromocene: 4 RCO 2 H + 2 Cr(C 5 H 5) 2 → Cr 2 (O 2 CR) 4 + 4 C 5 H 6. This method provides anhydrous derivatives in a straightforward manner. [8] Because it is so easily prepared, Cr 2 (OAc) 4 (H 2 O) 2 is a
The solution has 1 mole or 1 equiv Na +, 1 mole or 2 equiv Ca 2+, and 3 mole or 3 equiv Cl −. An earlier definition, used especially for chemical elements , holds that an equivalent is the amount of a substance that will react with 1 g (0.035 oz) of hydrogen , 8 g (0.28 oz) of oxygen , or 35.5 g (1.25 oz) of chlorine —or that will displace ...
Chromium(III) sulfide is the inorganic compound with the formula Cr 2 S 3. It is a brown-black solid. It is a brown-black solid. Chromium sulfides are usually nonstoichiometric compounds , with formulas ranging from CrS to Cr 0.67 S (corresponding to Cr 2 S 3 ).
The term molality is formed in analogy to molarity which is the molar concentration of a solution. The earliest known use of the intensive property molality and of its adjectival unit, the now-deprecated molal, appears to have been published by G. N. Lewis and M. Randall in the 1923 publication of Thermodynamics and the Free Energies of Chemical Substances. [3]
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 ...