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2.159*10^-25
The mass of a barium atom is approximately 137 atomic mass units (u).
It depends on which isotope you are talking about. Bariuim-133, for instance, has 133 AMU. (Atomic Mass Units) Known isotopes of barium range from -112 to -153.
10 formula units
How many grams of NaCl are present in 8.39x10^22 formula units of NaCl?
K2O is potassium oxide. Formula mass = 94g32.6 g x 1 FU/94 g = 0.35 formula units
K2O is potassium oxide. Formula mass = 94g32.6 g x 1 FU/94 g = 0.35 formula units
5.68 mol MgO x 6.02E23 formula units / 1 mol = 3.42E24 Formula Units
The mass is 991,5 g.
2.159*10^-25
Assuming that the number "9.871023" would or should have been written as "9.87 X 1023" if the typographical resources to do so were available to the questioner: Avogadro's Number, which is the number of formula units in a mole of any material, is about 6.022 X 1023. The gram formula mass for aluminum oxide is 101.96. Therefore, the mass of the stated number of formula units of aluminum oxide is: 101.96(9.87/6.022) or about 164 grams, to the justified number of significant digits.
Na2O is sodium oxide. The 2 at the beginning means that there are two formula units of it.
7.2
1. The correct chemical formula of barium hydroxide is Ba(OH)2. 2. The molecule of barium hydroxide contain 2 oxygen atoms.
0.550 mole BaCl2 x 6.02x10^23 formula units/mole x 3 atoms/formula unit = 9.93x10^23 atoms
The mass of a barium atom is approximately 137 atomic mass units (u).
Barium nitride is Ba3N2 (from the rules of ionic bonding). Its molar mass is 439 grams/mole (from the periodic table), so 18.8 grams of it is 0.0428 moles (by algebraic direct proportion). Multiply this by Avogadro's number (6.02x1023; the number of particles in 1 mole) and you get 2.58x1022 formula units of barium nitride, and there are 2 nitrogen atoms per formula unit, so double it to 5.16x1022 atoms of nitrogen.