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1.12 x 10^22 atoms PFirst determine the number of moles in the 0.577 g sample of phosphorus, determine the number of moles in the sample. Then multiply the moles by 6.022x10^23 atoms/mol.0.577 g P x (1 mol P/30.974 g P) x (6.022x10^23 atoms P/1 mol P) = 1.12 x 10^22 atoms P
1.3 mol
The mass of phosphorus of any sample of calcium phosphate is the mass of the same multiplied by the percentage that phosphorus makes up of that sample. (mass of sample) x (mass of phosphorus/total mass) Therefore we must look at the chemical formula of the substance in question: Ca3(PO4)2. From this we can see that there are 2 phosphorus atoms attributing mass to the total molecule. The formula becomes: 500 g x 2x30.97 g/mol/310.17 g/mol = 99.8 g molar mass of phosphorus: 30.97 g/mol molar mass of calcium phosphate: 310.17 g/mol total mass: 500 g
48,177 134 32.1023 atoms
0.63 mol of (NH4)2SO4 contain 3,978.10e23 hydrogen atoms.
The number of phosphorus atoms is 5,326095.10e23.
The number of atoms is 39,746.10e23.
4.91 mol * 6.02214129(27)×1023 / mol = 2.96 ×1024
158kg P* 1000g/1 Kg * 1 mol P/30.974 g * 6.022e23 P Atom/mol P = 3.07e27
12 (g) / 31 (g/mol) = 0.387 g / (g/mol) = 0.39 mol of P atoms
1.12 x 10^22 atoms PFirst determine the number of moles in the 0.577 g sample of phosphorus, determine the number of moles in the sample. Then multiply the moles by 6.022x10^23 atoms/mol.0.577 g P x (1 mol P/30.974 g P) x (6.022x10^23 atoms P/1 mol P) = 1.12 x 10^22 atoms P
the constant Mole (mol): 6.02 x 10^23 are how many atoms you have per mol so the answer can be 7 mol atoms or 6.02 x 10^23 atoms per mol x 7 actual answer is 4.214 X10^24 atoms in 7 mol
A mol = 6,022x10^23 atoms 1,5 mol = 9,033x10^23 atoms Always.
There are 1.204 x 1023 atoms in .200 mol of Pb.
There are 1.41 e24 atoms of Na in 2.35 mol of NaCl.
0.45 mol BaSO4 have 2,698.10e23 sulfur atoms.
1.3 mol