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Number of particles=number of moles x avogadro constant = 25.9 x 6.02 x 1023
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What is the mass of 2.25 moles of iron?
The answer is 125,65 g.
How many grams of H 2O will be produced if 750 grams of Fe are produced?
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 mass in grams in 1.00 molar mass FE?
What is the chemical 'FE'. Do you mean 'Fe'. If so to answer your question . The molar mass of iron (Fe) is 55.845
How many Cl ions are present in 50.0 g FeCl3?
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.
Moles are there in 82.5 grams of iron?
To determine the number of moles in 82.5 grams of iron, you need to divide the given mass by the molar mass of iron, which is approximately 55.85 g/mol. By dividing 82.5 grams by 55.85 g/mol, you would find approximately 1.48 moles of iron.
What minimum mass of HCl in grams would you need to dissolve a 2.2 g iron bar on a padlock?
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
How many atoms are in 10g of Fe?
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.
What is the maximum mass of iron metal if 50.0 grams of ironIII oxide is mixed with 50.0 grams of aluminum?
Fe2O3 + 2Al --> 2Fe + Al2O3Before:50.0g + 50.0g > 0.0g + (not important)159.69(g/mol) + 26.98(g/mol)In mol (before reaction):+0.3131 mol + 1.853 mol (excess)Reaction (used reactant > formed Fe):-0.3131 mol - 0.6262 mol > + 0.6262 mol FeRemaining (= before - used):0.0 mol Fe2O3 + 1.227 mol Al > 0.6262 mol Fe, this should be multiplied by the molar mass of Fe to get mass in grams: 0.6262 (molFe) * 55.85 (g/molFe) = 34.97 = 35.0 g Fe
What is the mass of 200 moles 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.
How many iron atoms are present in 55.845grams of Iron?
Amount of Fe = 55.845/55.845 = 1mol There is 1 mol of Fe in a 55.845g sample. 1 mol of Fe contains 6.02 x 1023 atoms (avogadro constant). Therefore there are 6.02 x 1023 atoms in 55.845g of iron.
What is the percentage of Fe in iron ammonium sulfate hexahydrate?
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%
What is the weight percent of iron in 2FeO3?
FeO3 = 103.845 g/mol Fe = 55.845 g/mol (55.845 g/103.845 g) x 100% = 53.8% Fe in 2FeO3
What is the mass of 2.25 mol of the element iron fe?
The answer is 125,65 g.
What is the molecular weight of nitroprusside?
The molar mass of Nitroprusside:Na2[Fe(CN)5NO] is 261.92 g/mol (anhydrous)Na2[Fe(CN)5NO].[H2O]2 is 297.95 g/mol (as dihydrate)
How many moles of nitrogen atoms are present in 53.55 g of FeNO32?
Molar mass of Fe(NO3)2 is 55.85 + 2(14.00 + 3(16.00)) = 179.85 g/mol Therefore, number of moles of Fe(NO3)2 present is 53.55/179.85 = 0.2977 mol For each molecule of Fe(NO3)2, there are two atoms of nitrogen associated with it. Therefore, there are 0.2977*2 = 0.5954 mol of nitrogen atoms
Determine the number of atoms in 3.75 mol Fe?
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.
If 1.164g of iron fillings reacts with chlorine gas to give 3.384 g of iron chloride what is the empirical formula of the compound Use the mole ratio method.?
1.164 g Fe / 55.85 g/mol = 0.02084 mol Fe (3.384 g - 1.164 g) Cl / 35.45 g/mol = 0.06262 mol Cl ratio of Fe : Cl = 1 : 3 empirical formula = FeCl3
