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To find the number of atoms in 1.4 moles of phosphorus trifluoride (PF₃), first note that each molecule of PF₃ contains 1 phosphorus atom and 3 fluorine atoms, totaling 4 atoms per molecule. Therefore, in 1.4 moles of PF₃, there are (1.4 , \text{mol} \times 4 , \text{atoms/molecule} = 5.6 , \text{mol of atoms}). Since 1 mole contains approximately (6.022 \times 10^{23}) entities (Avogadro's number), the total number of atoms is (5.6 , \text{mol} \times 6.022 \times 10^{23} , \text{atoms/mol} \approx 3.37 \times 10^{24} , \text{atoms}).
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How many atoms of phosphorus are in 8.90 mol of copperII phosphate?
To find the number of phosphorus atoms in 8.90 mol of copper(II) phosphate (Cu₃(PO₄)₂), we first identify that each formula unit contains 2 phosphorus (P) atoms. Thus, in 8.90 mol of copper(II) phosphate, the total number of phosphorus atoms is calculated as follows: 8.90 mol × 2 P/mol = 17.8 mol of phosphorus atoms. To convert moles to atoms, we multiply by Avogadro's number (approximately (6.022 \times 10^{23}) atoms/mol): 17.8 mol × (6.022 \times 10^{23}) atoms/mol ≈ (1.07 \times 10^{24}) phosphorus atoms.
How many atoms of phosphorus are in a 0.577 g sample?
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
How many atoms in 5.18 g P?
To find the number of atoms in 5.18 grams of phosphorus (P), first determine the molar mass of phosphorus, which is approximately 30.97 g/mol. Then, calculate the number of moles in 5.18 g by dividing the mass by the molar mass: 5.18 g / 30.97 g/mol ≈ 0.167 moles. Finally, multiply the number of moles by Avogadro's number (approximately (6.022 \times 10^{23}) atoms/mol) to find the number of atoms: 0.167 moles × (6.022 \times 10^{23}) atoms/mol ≈ (1.01 \times 10^{23}) atoms.
2. Calculate the number of moles of phosphorus in 15.95 g of tetraphosphorus decaoxide.?
To calculate the number of moles of phosphorus in 15.95 g of tetraphosphorus decaoxide (P₄O₁₀), first determine its molar mass. The molar mass of P₄O₁₀ is approximately 284 g/mol (4 phosphorus atoms at 31 g/mol each and 10 oxygen atoms at 16 g/mol each). Next, use the formula: moles = mass (g) / molar mass (g/mol). So, moles of P₄O₁₀ = 15.95 g / 284 g/mol ≈ 0.0562 moles. Since there are 4 moles of phosphorus in each mole of P₄O₁₀, multiply by 4 to find the moles of phosphorus: 0.0562 moles × 4 ≈ 0.2248 moles of phosphorus.
How many grams of phosphorus are in 500 grams of calcium phosphate?
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
How many atoms are in 1.4 mol of phosphorus trifluoride (PF3)?
1.4 mol of phosphorus trifluoride (PF3) would contain 8.4 x 10^23 molecules, since each molecule of PF3 contains 4 atoms (1 phosphorus atom and 3 fluorine atoms). So, there would be 33.6 x 10^23 atoms in 1.4 mol of PF3.
How many atoms of phosphorus are in 3.30 mol of copper (ll) phosphate?
There are 1 mol of phosphorus atoms in 1 mol of copper (II) phosphate. Therefore, in 3.30 mol of copper (II) phosphate, there are 3.30 mol of phosphorus atoms, which is equivalent to 3.30 x 6.022 x 10^23 = 1.97 x 10^24 atoms of phosphorus.
How many atoms of phosphorus are in 4.40 mol of copper(II) phosphate?
There are 1 atom of phosphorus in each formula unit of copper(II) phosphate, which is Cu3(PO4)2. Therefore, in 4.40 mol of copper(II) phosphate, there are 4.40 mol of phosphorus atoms, which is 4.40 x 6.022 x 10^23 atoms.
How many phosphorus atoms does it take to equal 30.973 grams?
To determine the number of phosphorus atoms in 30.973 grams, you would first convert the mass to moles using the molar mass of phosphorus (30.973 g/mol). Then, you would use Avogadro's number (6.022 x 10^23 atoms/mol) to find the number of phosphorus atoms, which would be 30.973 grams / 30.973 g/mol * 6.022 x 10^23 atoms/mol.
How many atoms are in 5.22 g of phosporous?
To find the number of atoms in 5.22 g of phosphorus, you first need to determine the number of moles of phosphorus by dividing the given mass by the molar mass of phosphorus (31.0 g/mol). From there, you can use Avogadro's number (6.022 x 10^23 atoms/mol) to convert moles to atoms.
How many moles of phosphorus atoms are in a 100 g sample of phosphorus?
The gram atomic mass of phosphorus is 30.9738, and by definition, a mole of such atoms contains Avogadro's Number of atoms. Therefore, 100 g of phosphorus contains 100/30.9738 or 3.23 moles, to the justified number of significant digits.
How many phosphorus atoms are contained in 158 kg of phosphorus?
To calculate the number of phosphorus atoms in 158 kg of phosphorus, we first need to determine the number of moles of phosphorus in 158 kg using the molar mass of phosphorus. Then we can use Avogadro's number (6.022 x 10^23 atoms per mole) to convert moles of phosphorus to atoms. The final calculation will give us the total number of phosphorus atoms in 158 kg.
How many grams of fluorine are contained in 5 molecules of boron trifluoride?
To calculate the number of grams of fluorine in 5 molecules of boron trifluoride, you need to first determine the molar mass of boron trifluoride (BF3). Boron trifluoride has one boron atom and three fluorine atoms, so the molar mass is ~ 67.8 g/mol. Since each molecule of boron trifluoride contains three fluorine atoms, the total mass of fluorine in 5 molecules would be 3 times the molar mass of fluorine (approximately 19.0 g/mol) times 5.
How many grams are in one mole of Bromine trifluoride?
The molar mass of Bromine trifluoride is approximately 126.893 g/mol. Therefore, one mole of Bromine trifluoride contains 126.893 grams.
How many grams are in the 1.204 1020 atoms of phosphorus used to coat your television screen?
To calculate the grams of phosphorus, you need to know the molar mass of phosphorus and then use Avogadro's number to convert from atoms to grams. The molar mass of phosphorus is approximately 30.97 g/mol. Therefore, you can calculate the grams of phosphorus using this information.
How many atoms of phosphorus are in a 0.577 g sample?
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
How many molecules of nitrogen trifluoride are present in 4.91 moles of nitrogen trifluoride?
4.91 mol * 6.02214129(27)×1023 / mol = 2.96 ×1024
