0
Number of particles=number of moles x avogadro constant = 25.9 x 6.02 x 1023
Wiki User
∙ 13y ago
Add your answer:
Earn +20 pts
What is the mass of 2.25 moles of iron?
The answer is 125,65 g.
What is Fe?
'Fe' is iron. The symbol (Fe) comes from the Latin for iron, which is 'Ferrum'.
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 grams of H 2O will be produced if 750 grams of Fe are produced?
322 grams.
How many unpaired electrons are in Iron-III?
There are 5 unpaired electrons in Fe^3+ in its ground state.
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?
Molar mass of iron = 55.845g/mol (atomic weight in grams/mol) 1mol Fe atoms = 6.022 x 1023 atoms Fe 10g Fe x 1mol/55.845g x 6.022 x 1023 atoms/mol = 1.078 x 1023 atoms
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?
200 (mol) * 56.0 (g/mol) = 11,200.0 grams
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)
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.
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
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
