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The amount of particles (any kind) in ONE mole (of any substance) is always equal to Avogadro's number: 6.02*10+23
(This is the definition of a 'Mole'. It is just a number like a 'dozen' -12- or 'gross' -144-, though much larger. There is nothing 'chemical' in this number, however)
So, here is your answer: 0.56 mole = 0.56 * 6.02*10+23 = 3.37*10+23
Wiki User
∙ 13y ago
There are 1 mole of iron atoms in approximately 56g of iron, since the Atomic Mass of iron is 56g/mol.
Wiki User
∙ 13y agoPretty close to one mole, Avogadro's number, of atoms.
56 grams iron (1 mole Fe/55.85 grams)(6.022 X 10^23/1 mole Fe)
= 6.038 X 10^23 atoms of Fe ( call it 6.04 X 10^23 )
Wiki User
∙ 15y agoThe atomic mass oof iron is 56a.m.u so 56g iron means 1 mole of iron.
Wiki User
∙ 10y ago1.00274 moles
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Which contains more atoms 56g of Fe or 16g of S?
There are more atoms of sulfur in 16 grams than there are atoms of iron in 56 grams.
How much iron sulphide will be formed if 56g of iron and 40g of sulphur are mixed?
Iron(II) sulfide is formed by the reaction of iron and sulfur as follows: Fe + S --> FeS To determine the amount of iron(II) sulfide formed, we need to consider the limiting reactant, which is sulfur in this case. The molar mass of iron(II) sulfide is 87.91 g/mol. Therefore, if 40g of sulfur reacts, it will form 40g / (32.06g/mol) = 1.25 moles of iron(II) sulfide, which is equivalent to 1.25 x 87.91 = 109.89g. So, 109.89g of iron sulfide will be formed.
What is the percent yield for iron if the reaction of 65.0 g of iron oxide produces 33.0 g of iron?
The molar mass of FeO is 71.85 g/mol, and the molar mass of Fe is 55.85 g/mol. Using the reaction's stoichiometry, we find that 65.0 g of FeO corresponds to 45.85 g of Fe. Therefore, the percent yield of Fe is (33.0 g / 45.85 g) x 100 = 71.96%.
What is the significant figures for 56g?
The significant figures for 56g are two, as there are two non-zero digits in the number.
What is the volume of 56g of nitrogen gas at 750mmHg and 25c?
To find the volume of a gas, we can use the ideal gas law: PV = nRT. First, calculate the moles of nitrogen using the given mass and molar mass. Then, rearrange the ideal gas law to solve for volume: V = nRT/P. Plug in the values for n (moles), R (ideal gas constant), T (temperature in Kelvin), and P (pressure) to find the volume.
Calculate the number of moles in 112 g of iron?
To calculate the number of moles in 112 g of iron, divide the given mass (112 g) by the molar mass of iron, which is approximately 55.85 g/mol. So, 112 g / 55.85 g/mol = approximately 2 moles of iron.
How many moles of CC14 are present in 56g?
This is carbon tetra chloride. there are 0.3636 moles in this mass.
Which contains more atoms 56g of Fe or 16g of S?
There are more atoms of sulfur in 16 grams than there are atoms of iron in 56 grams.
What does 56g equals?
56g=0.56kg
How much does one mole of iron atoms weigh?
Use the equation; mass=moles*gramformulamass or m=n*gfm m=2*55.8 = 111.6g in two moles of Iron gfm or the molecular mass of a compound can be found by adding the Relative atomic masses of each element in the compound together. For example - Carbon dioxide CO2 The formula contains 1 Carbon atom and 2 Oxygen atoms (RAMs should be found in a datasheet/book or provided in the question. RAM = relative atomic mass) RAM Carbon = 12 RAM Oxygen = 16 gfm of CO2 = 12 + 32 = 44 or 1mole of CO2 = 44g
How much iron sulphide will be formed if 56g of iron and 40g of sulphur are mixed?
Iron(II) sulfide is formed by the reaction of iron and sulfur as follows: Fe + S --> FeS To determine the amount of iron(II) sulfide formed, we need to consider the limiting reactant, which is sulfur in this case. The molar mass of iron(II) sulfide is 87.91 g/mol. Therefore, if 40g of sulfur reacts, it will form 40g / (32.06g/mol) = 1.25 moles of iron(II) sulfide, which is equivalent to 1.25 x 87.91 = 109.89g. So, 109.89g of iron sulfide will be formed.
What is 130 percent of 56g?
130% of 56g = 130% * 56 = 1.3 * 56 = 72.8g
What is the mass of one mole of iron sulphate?
In one mole of each element there is... Fe - 56g O - 16g S - 32g Th equation is Fe2(SO4)3 56g x 2 = 112g 32g x 3 = 96g 16g x 12 = 192g 112g + 96g + 192g = 400g 400g
What is the percent yield for iron if the reaction of 65.0 g of iron oxide produces 33.0 g of iron?
The molar mass of FeO is 71.85 g/mol, and the molar mass of Fe is 55.85 g/mol. Using the reaction's stoichiometry, we find that 65.0 g of FeO corresponds to 45.85 g of Fe. Therefore, the percent yield of Fe is (33.0 g / 45.85 g) x 100 = 71.96%.
What is the significant figures for 56g?
The significant figures for 56g are two, as there are two non-zero digits in the number.
How many carbohydrates is a lollypop?
a lollypop has 24 carbs in it
What is the volume of 56g of nitrogen gas at 750mmHg and 25c?
To find the volume of a gas, we can use the ideal gas law: PV = nRT. First, calculate the moles of nitrogen using the given mass and molar mass. Then, rearrange the ideal gas law to solve for volume: V = nRT/P. Plug in the values for n (moles), R (ideal gas constant), T (temperature in Kelvin), and P (pressure) to find the volume.
