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The molar mass of Fe(NO3)2 (iron(II) nitrate) is calculated by adding the atomic masses of all the atoms in the formula: Fe (iron) has a molar mass of approximately 55.85 g/mol, N (nitrogen) has a molar mass of approximately 14.01 g/mol, and O (oxygen) has a molar mass of approximately 16.00 g/mol. Therefore, the molar mass of Fe(NO3)2 is around 179.86 g/mol.
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What mass of ironIIInitrate is needed for a chemical reaction that requires 6.00 moles of FeNO33?
To determine the mass of iron(II) nitrate needed for 6.00 moles of Fe(NO3)2, you first need to calculate the molar mass of Fe(NO3)2. Fe(NO3)2 has a molar mass of approximately 179.86 g/mol. Therefore, the mass needed would be 6.00 moles * 179.86 g/mol ≈ 1079.16 grams of Fe(NO3)2.
What is Fe(NO3)2?
Fe(NO3)2 is the chemical formula for iron(II) nitrate, which is a salt formed by the combination of iron(II) ions and nitrate ions. It is commonly used in analytical chemistry and as a precursor for the synthesis of other iron compounds.
What is the molar mass of Pb(NO3)2?
The molar mass of Pb(NO3)2 is calculated by adding up the atomic masses of each individual element in the compound. For Pb(NO3)2, the molar mass would be: Lead (Pb): 207.2 g/mol Nitrogen (N): 14.0 g/mol Oxygen (O): 16.0 g/mol Therefore, the molar mass of Pb(NO3)2 would be 207.2 + 2(14.0) + 6(16.0) = 331.2 g/mol.
Is Fe(NO3)2 Ionic or molecular?
Fe(NO3)2 is an ionic compound. Iron (Fe) is a metal and nitrate (NO3) is a polyatomic ion, so together they form an ionic bond in Fe(NO3)2.
How do you find the molar mass of lead (II) nitrate (Pb(NO3)2)?
To find the molar mass of lead (II) nitrate (Pb(NO3)2), you first calculate the individual atomic masses of each element in the compound (Pb, N, O). Then, add up the atomic masses of each element based on the subscripts in the formula (2 nitrogens and 6 oxygens in this case) to get the molar mass. In this case, the molar mass of Pb(NO3)2 would be 331.2 g/mol.
What is the molar mass of Fe(NO3)2?
The molar mass of anhydrous iron(II) nitrate is 179,91 g.
What mass of ironIIInitrate is needed for a chemical reaction that requires 6.00 moles of FeNO33?
To determine the mass of iron(II) nitrate needed for 6.00 moles of Fe(NO3)2, you first need to calculate the molar mass of Fe(NO3)2. Fe(NO3)2 has a molar mass of approximately 179.86 g/mol. Therefore, the mass needed would be 6.00 moles * 179.86 g/mol ≈ 1079.16 grams of Fe(NO3)2.
What is Fe(NO3)2?
Fe(NO3)2 is the chemical formula for iron(II) nitrate, which is a salt formed by the combination of iron(II) ions and nitrate ions. It is commonly used in analytical chemistry and as a precursor for the synthesis of other iron compounds.
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
The molar mass of CaCO3 is greater than the molar mass of CaNO32?
No, this statement is incorrect. The molar mass of CaCO3 (calcium carbonate) is 100.09 g/mol, while the molar mass of Ca(NO3)2 (calcium nitrate) is 164.08 g/mol. Therefore, the molar mass of Ca(NO3)2 is greater than that of CaCO3.
What is the molar mass of Pb(NO3)2?
The molar mass of Pb(NO3)2 is calculated by adding up the atomic masses of each individual element in the compound. For Pb(NO3)2, the molar mass would be: Lead (Pb): 207.2 g/mol Nitrogen (N): 14.0 g/mol Oxygen (O): 16.0 g/mol Therefore, the molar mass of Pb(NO3)2 would be 207.2 + 2(14.0) + 6(16.0) = 331.2 g/mol.
What is the formula of iron and nitrate?
Iron nitrates are: - Fe(II)(NO3)2 - Fe(III)(NO3)3
Is Fe(NO3)2 Ionic or molecular?
Fe(NO3)2 is an ionic compound. Iron (Fe) is a metal and nitrate (NO3) is a polyatomic ion, so together they form an ionic bond in Fe(NO3)2.
How do you find the molar mass of lead (II) nitrate (Pb(NO3)2)?
To find the molar mass of lead (II) nitrate (Pb(NO3)2), you first calculate the individual atomic masses of each element in the compound (Pb, N, O). Then, add up the atomic masses of each element based on the subscripts in the formula (2 nitrogens and 6 oxygens in this case) to get the molar mass. In this case, the molar mass of Pb(NO3)2 would be 331.2 g/mol.
How many molecules are there in 122 grams of Cu(NO3)2?
To find the number of molecules in 122 grams of Cu(NO3)2, we need to first calculate the molar mass of Cu(NO3)2. The molar mass of Cu(NO3)2 is approximately 187.55 g/mol. Next, we convert the given mass to moles using the molar mass. Finally, we use Avogadro's number (6.022 x 10^23) to find the number of molecules, which would be approximately 3.25 x 10^22 molecules.
What is the product of NO3 and iron II?
The product of NO3 and iron II is iron(II) nitrate, which has the chemical formula Fe(NO3)2.
How many grams of Cu(NO3)2 will be produced if you start with 4.2 grams of cu?
To determine the number of grams of Cu(NO3)2 produced, you need to consider the molar ratio between Cu(NO3)2 and Cu. Firstly, convert the 4.2 grams of Cu to moles using the molar mass of Cu. Then, use the balanced chemical equation to find the moles of Cu(NO3)2 produced. Finally, convert the moles of Cu(NO3)2 to grams using its molar mass.
