Number of particles=number of moles x avogadro constant = 25.9 x 6.02 x 1023
The answer is 125,65 g.
In the reaction of Fe with H₂O to produce FeO and H₂, the ratio is 3 moles of H₂O for every 1 mole of Fe. Since the molar mass of Fe is 56 g/mol and that of H₂O is 18 g/mol, we use these values to find that 750 grams of Fe will produce 750 * (3 * 18 / 56) = 857.14 grams of H₂O.
What is the chemical 'FE'. Do you mean 'Fe'. If so to answer your question . The molar mass of iron (Fe) is 55.845
To find the number of Cl ions in FeCl3, we first need to calculate the molar mass of FeCl3. Iron (Fe) has a molar mass of approximately 55.85 g/mol, and chlorine (Cl) has a molar mass of approximately 35.45 g/mol. Therefore, the molar mass of FeCl3 is 55.85 + (3 * 35.45) = 126.2 g/mol. Next, we determine how many moles of FeCl3 are present in 50.0 g by dividing the mass by the molar mass: 50.0 g / 126.2 g/mol ≈ 0.396 mol. Since there are 3 Cl ions in every FeCl3 molecule, there are approximately 0.396 mol * 3 = 1.19 mol of Cl ions. Finally, we use Avogadro's number (6.022 x 10^23 molecules/mol) to find the number of Cl ions: 1.19 mol * 6.022 x 10^23 Cl molecules/mol = approximately 7.16 x 10^23 Cl ions.
For this you need the atomic mass of Fe. Take the number of grams and divide it by the atomic mass. Multiply by one mole for units to cancel.82.5 moles Fe / (55.9 grams) = 1.48 moles Fe
3.8 g Fe * 1 mol Fe/55.85 g Fe (molar mass) = .0680 mol Fe .0680 mol Fe * 2 mol HBr/1 mol Fe (found in formula Fe+2HBr=>FeBr2+H2)=.136 mol HBr .136 mol HBr*80.912 g HBr/1 mol HBr=11.004 g HBr (or 11 using 2 sig figs) And the mass of H2 that is produced is 0.14 g
To determine the number of atoms in 10g of Fe, you first need to calculate the number of moles of Fe using its molar mass (55.85 g/mol). Then, you can use Avogadro's number (6.022 x 10^23 atoms/mol) to find the number of atoms in those moles of Fe. Finally, multiply the number of moles by Avogadro's number to get the total number of atoms in 10g of Fe.
The molar mass of Fe (iron) is 55.85 g/mol. Therefore, the mass of 200 moles of Fe would be 200 moles × 55.85 g/mol = 11,170 g or 11.17 kg.
A lot!! 850 moles iron (6.022 X 10^23/1 mole Fe) = 5.12 X 10^26 atoms of iron
The answer is 125,65 g.
Well, honey, it's simple math. The balanced chemical equation tells us that 4 moles of Al2O3 are produced for every 3 moles of Fe. So if you start with 0.60 mol of Fe, you just set up a simple ratio and find that you'll produce 0.80 mol of Al2O3. Easy peasy lemon squeezy!
6,78.1022 molecules of glucose 2,14388229924.1024 iron atoms 1,25.1025 zinc atoms
Since a mole of a metal is generally considered to be Avogadro's Number of atoms of the metal, the answer is 3.5 times Avogadro's Number or 2.1 X 1024 atoms, to the justified number of significant digits.
To determine the number of atoms in 12.5 g of Fe, you need to first calculate the number of moles of Fe using its molar mass (55.84 g/mol). Then, use Avogadro's number (6.022 x 10^23 atoms/mol) to convert moles to atoms.
The molar mass of Fe2O3 is 159.69 g/mol, and the molar mass of Fe is 55.85 g/mol. Theoretical yield of Fe = (42.0 g Fe) / (55.85 g/mol) x 2 = 1.50 mol Fe. Percent yield = (actual yield / theoretical yield) x 100 = (42.0 g / 1.50 mol x 55.85 g/mol) x 100 = 63.2%.
To determine the amount of C required to react with Fe, we need to use the balanced chemical equation. For example, if the balanced equation is Fe + C -> FeC, and the molar mass of Fe is 55.85 g/mol and C is 12.01 g/mol, then 55.85 g Fe is equal to 12.01 g C. From this, you can calculate the amount of C needed to react with 286.5 g of Fe.
14% FeThe formula for iron ammonium sulfate hexahydrate is (NH4)2Fe(SO4)2·6H2O, which can also be written as FeH20N2O14S2.To determine the percentage of Fe in the compound, divide the mass of Fe by the mass of the compound and multiply by 100. The molar mass of Fe is 56 g/mol. The molar mass of the compound is 392 g/mol. There is only one Fe atom in the formula, so the mass of Fe is 56 g/mol.%Fe = (56 g/mol)/(392 g/mol) x 100 = 14%