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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)2molecular weight. Molar mass of Fe(NO3)2= 179.8548 g/mol. This compound is also known as Iron(II) Nitrate. Convert grams Fe(NO3)2to moles or moles Fe(NO3)2to grams.
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.
Give the name and calculate the molar mass for Fe NO3 3?
I presume you mean 'Fe(NO3)3'. Note the use of brackets to indicate the number of nitrate anions. Otherwise the 'stand alone' suffix '3' is meaningless. Or wrongly confused as '33' oxygen atoms'. Note the use of Roman Numerals to indicate the oxidation state of iron. Fe(NO3)3 is Iron(III)nitrate or Ferric Nitrate. Molar Mass Fe x 1 = 56 x 1 = 56 N x 3 = 14 x 3 = 42 O x 3 x 3 = 16 x 9 = 144 56 + 42 + 144 = 242 (The molar mass). NB The 'N x 3' comes from the three nitrogen atoms, one each in the THREE nitrate anions. Similarly The 'O x 3 x 3 comes from three oxygen atoms, in each nitrate anion. There being three nitrate anions, means that there 3 x 3 = 9 oxygen atoms in the molecule. NNB Careful with the nomenclature. If there are only TWO nitrate anions present in the molecule , then the formula is 'Fe(NO3)2, and the name(s) are Iron(II)Nitrate or Ferrous Nitrate. NNNB 'Fe' is the chemical symbol for Iron. It comes from the Latin for Iron, which is 'Ferrum (Fe)'.
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.
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)2molecular weight. Molar mass of Fe(NO3)2= 179.8548 g/mol. This compound is also known as Iron(II) Nitrate. Convert grams Fe(NO3)2to moles or moles Fe(NO3)2to grams.
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
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.
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 formula of iron and nitrate?
Iron nitrates are: - Fe(II)(NO3)2 - Fe(III)(NO3)3
Give the name and calculate the molar mass for Fe NO3 3?
I presume you mean 'Fe(NO3)3'. Note the use of brackets to indicate the number of nitrate anions. Otherwise the 'stand alone' suffix '3' is meaningless. Or wrongly confused as '33' oxygen atoms'. Note the use of Roman Numerals to indicate the oxidation state of iron. Fe(NO3)3 is Iron(III)nitrate or Ferric Nitrate. Molar Mass Fe x 1 = 56 x 1 = 56 N x 3 = 14 x 3 = 42 O x 3 x 3 = 16 x 9 = 144 56 + 42 + 144 = 242 (The molar mass). NB The 'N x 3' comes from the three nitrogen atoms, one each in the THREE nitrate anions. Similarly The 'O x 3 x 3 comes from three oxygen atoms, in each nitrate anion. There being three nitrate anions, means that there 3 x 3 = 9 oxygen atoms in the molecule. NNB Careful with the nomenclature. If there are only TWO nitrate anions present in the molecule , then the formula is 'Fe(NO3)2, and the name(s) are Iron(II)Nitrate or Ferrous Nitrate. NNNB 'Fe' is the chemical symbol for Iron. It comes from the Latin for Iron, which is 'Ferrum (Fe)'.
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 equation would look like: 2(NO3) + Fe --> Fe(NO3)2 the 2 in front of the NO3 is there to balance the equation.
