Atomic Mass of Fe: 55.8g/mol
Atomic Mass of O: 16g/mol
Molecular mass of Fe2O3: 2(55.8)+3(16) = 159.6g/mol
mass = Molecular mass x number of moles
mass = 159.6g/mol x 0.7891mol = 125.94g
Atomic Mass of Fe: 55.8g/mol
Atomic mass of O: 16g/mol
Molecular mass of Fe2O3: 2(55.8)+3(16) = 159.6g/mol
mass = Molecular mass x number of moles
mass = 159.6g/mol x 0.7891mol = 125.94g
Adding together the mass of two irons and three oxygen.....,251 grams Fe2O3 (1 mole Fe2O3/159.7 grams)= 1.57 moles iron II oxide ( also known as ferric oxide )===================================
Rust has a chemical formula of Fe2O3. Ferric oxide has a molar mass of 159.69 grams per mol and a density of 5.26 grams per cubic centimeter.
Atomic mass of Fe: 55.8g/mol Atomic mass of O: 16g/mol Molecular mass of Fe2O3: 2(55.8)+3(16) = 159.6g/mol mass = Molecular mass x number of moles mass = 159.6g/mol x 0.7891mol = 125.94g
Atomic Mass of Fe: 55.8g/mol Atomic mass of O: 16g/mol Molecular mass of Fe2O3: 2(55.8)+3(16) = 159.6g/mol mass = Molecular mass x number of moles mass = 159.6g/mol x 0.7891mol = 125.94g
The molar mass of anhydrous iron(II) nitrate is 179,91 g.
Adding together the mass of two irons and three oxygen.....,251 grams Fe2O3 (1 mole Fe2O3/159.7 grams)= 1.57 moles iron II oxide ( also known as ferric oxide )===================================
Rust has a chemical formula of Fe2O3. Ferric oxide has a molar mass of 159.69 grams per mol and a density of 5.26 grams per cubic centimeter.
That is the chemical formula. The name would be iron (III) oxide, or ferric oxide in the old system.
Atomic mass of Fe: 55.8g/mol Atomic mass of O: 16g/mol Molecular mass of Fe2O3: 2(55.8)+3(16) = 159.6g/mol mass = Molecular mass x number of moles mass = 159.6g/mol x 0.7891mol = 125.94g
Atomic Mass of Fe: 55.8g/mol Atomic mass of O: 16g/mol Molecular mass of Fe2O3: 2(55.8)+3(16) = 159.6g/mol mass = Molecular mass x number of moles mass = 159.6g/mol x 0.7891mol = 125.94g
The molar mass of anhydrous iron(II) nitrate is 179,91 g.
There are two atoms of iron and three atoms of oxygen in the compound Fe2O3. The mass percent of iron is 69.943%
For this you need the atomic (molecular) mass of Fe2(SO4)3. Take the number of grams and divide it by the atomic mass. Multiply by one mole for units to cancel. Fe2(SO4)3=400.1 grams768 grams Fe2(SO4)3 / (400.1 grams) = 1.92 moles Fe2(SO4)3
14.2g Fe2O3 (1mol Fe2O3/159.7g(2mol Fe/1mol Fe2O3) = 0.178 moles Fe
Mass of Fe=(Mass of Fe2O3)(Mr Fe/ Mr Fe2O3)
6g hydrogen would be required for 160g ferric oxide in this reaction. The relative atomic weights of the elements are: Hydrogen - 1 Oxygen - 16 Iron - 56 giving the relative atomic weights of the compounds (on the left of the equation): Fe2O3 = 56×2 + 16×3 = 160 3H2 = 3×(1×2) = 6 So for every 160 units of mass of iron III oxide there will be 6 units of mass of hydrogen required. → for 160g of iron III oxide ÷ 160 × 6 = 6 g of hydrogen.
FeNo2 is iron nitrite.Answer 2. Ferrous Nitrite or iron Nitrite (II)would be Fe(NO2)2.Ferric Nitrite or Iron Nitrite (III) would be Fe(NO2)3.