0
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 grams
768 grams Fe2(SO4)3 / (400.1 grams) = 1.92 moles Fe2(SO4)3
What else can I help you with?
How many moles are in 233.2 g iron Fe?
233,2 g iron Feis equivalent to 4,176 moles.
How many moles are in 23 g of Fe?
To find the number of moles in 23 g of Fe, first find the molar mass of Fe by looking up the atomic weight on the periodic table. Fe has a molar mass of approximately 55.85 g/mol. Divide the given mass by the molar mass to find the number of moles: 23 g Fe / 55.85 g/mol = approximately 0.41 moles of Fe.
How many moles are I am 223.2 g iron (Fe)?
To find the number of moles of iron (Fe) in 223.2 g, you can use the formula: moles = mass (g) / molar mass (g/mol). The molar mass of iron is approximately 55.85 g/mol. Thus, moles of iron = 223.2 g / 55.85 g/mol ≈ 3.99 moles.
How many moles are in 103.56 g of Fe3(PO4)2?
To find the number of moles in 103.56 g of Fe₃(PO₄)₂, first calculate its molar mass. The molar mass of Fe₃(PO₄)₂ is approximately 357.43 g/mol. Using the formula: moles = mass (g) / molar mass (g/mol), we get: moles = 103.56 g / 357.43 g/mol ≈ 0.29 moles.
If 250.0 g of Fe2O3 are used how many grams of iron can be produced?
To determine how many grams of iron can be produced from 250.0 g of Fe₂O₃, we first need to use the molar mass of Fe₂O₃, which is approximately 159.69 g/mol. The balanced chemical reaction for the reduction of Fe₂O₃ to iron is: Fe₂O₃ → 2 Fe + 1.5 O₂. From the stoichiometry of the reaction, 1 mole of Fe₂O₃ produces 2 moles of Fe. Thus, 250.0 g of Fe₂O₃ corresponds to about 1.56 moles, yielding approximately 3.12 moles of Fe, which is about 174.0 g of iron.
The formula for rust can be represented by Fe2O3 How many moles of Fe are present in 14.2 g of the compound?
To find the number of moles of Fe in 14.2 g of Fe2O3, we need to use the molar mass of Fe2O3 (molecular weight = 159.69 g/mol) and the ratio of Fe to Fe2O3. There are 2 moles of Fe in 1 mole of Fe2O3, so we find the moles of Fe in 14.2 g of Fe2O3 by: (14.2 g / 159.69 g/mol) * 2 = 0.249 moles of Fe.
How many moles are in 233.2 g iron Fe?
233,2 g iron Feis equivalent to 4,176 moles.
How many moles are in 23 g of Fe?
To find the number of moles in 23 g of Fe, first find the molar mass of Fe by looking up the atomic weight on the periodic table. Fe has a molar mass of approximately 55.85 g/mol. Divide the given mass by the molar mass to find the number of moles: 23 g Fe / 55.85 g/mol = approximately 0.41 moles of Fe.
How many moles are I am 223.2 g iron (Fe)?
To find the number of moles of iron (Fe) in 223.2 g, you can use the formula: moles = mass (g) / molar mass (g/mol). The molar mass of iron is approximately 55.85 g/mol. Thus, moles of iron = 223.2 g / 55.85 g/mol ≈ 3.99 moles.
How many moles are in 103.56 g of Fe3(PO4)2?
To find the number of moles in 103.56 g of Fe₃(PO₄)₂, first calculate its molar mass. The molar mass of Fe₃(PO₄)₂ is approximately 357.43 g/mol. Using the formula: moles = mass (g) / molar mass (g/mol), we get: moles = 103.56 g / 357.43 g/mol ≈ 0.29 moles.
How many moles are in 233.2 g iron (Fe)?
To find the number of moles in 233.2 g of iron (Fe), you need to divide the given mass by the molar mass of iron, which is approximately 55.85 g/mol. So, 233.2 g ÷ 55.85 g/mol ≈ 4.17 moles of iron.
If 250.0 g of Fe2O3 are used how many grams of iron can be produced?
To determine how many grams of iron can be produced from 250.0 g of Fe₂O₃, we first need to use the molar mass of Fe₂O₃, which is approximately 159.69 g/mol. The balanced chemical reaction for the reduction of Fe₂O₃ to iron is: Fe₂O₃ → 2 Fe + 1.5 O₂. From the stoichiometry of the reaction, 1 mole of Fe₂O₃ produces 2 moles of Fe. Thus, 250.0 g of Fe₂O₃ corresponds to about 1.56 moles, yielding approximately 3.12 moles of Fe, which is about 174.0 g of iron.
What is the mass of 2.25 moles of iron?
The answer is 125,65 g.
How many grams of Fe can be produced when 10.0 g of Al is reacted with an unlimited supply of Fe2o3?
To determine how many grams of Fe can be produced from 10.0 g of Al reacting with Fe2O3, we first need the balanced chemical equation for the reaction: [ 4Al + 3Fe2O3 \rightarrow 4Fe + 6Al2O3 ] From the equation, 4 moles of Al produce 4 moles of Fe. The molar mass of Al is approximately 27 g/mol, so 10.0 g of Al corresponds to about 0.37 moles of Al. This produces an equivalent of 0.37 moles of Fe. Given that the molar mass of Fe is about 56 g/mol, the mass of Fe produced is approximately (0.37 , \text{moles} \times 56 , \text{g/mol} \approx 20.72 , \text{g}).
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 moles of Fe are present in 30 grams in rust?
This amount may be different because rust is not a clearly definite compound.
How many atoms of Fe are in 12.5 g Fe?
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.
