If 507 g FeCL2 were used up in the reaction FeCL2 + 2NaOH > Fe(OH)@(s) + 2NaCL, how many grams of Fe(OH)2 would be formed?
mols FeCl2 = grams/molar mass
Using the coefficients in the balanced equation, convert mols FeCl2 to mols Fe(OH)2.
Now convert mols Fe(OH)2 to grams. g = mols x molar mass = ?
654
To determine the grams of Fe(OH)2 formed in the reaction, we need to use stoichiometry.
From the balanced equation:
1 mole of FeCl2 reacts with 2 moles of NaOH to produce 1 mole of Fe(OH)2.
First, we need to convert grams of FeCl2 to moles:
Molar mass of FeCl2 = atomic mass of Fe + (2 * atomic mass of Cl)
= 55.85 g/mol + (2 * 35.45 g/mol)
= 55.85 g/mol + 70.90 g/mol
= 126.75 g/mol
Moles of FeCl2 = grams of FeCl2 / molar mass of FeCl2
= 507 g / 126.75 g/mol
= 4 moles
Now, we can use the stoichiometry to determine moles of Fe(OH)2:
Moles of Fe(OH)2 = moles of FeCl2 * (1 mole of Fe(OH)2 / 1 mole of FeCl2)
= 4 moles * (1 mole / 1 mole)
= 4 moles
Finally, we can convert moles of Fe(OH)2 to grams:
Molar mass of Fe(OH)2 = atomic mass of Fe + (2 * atomic mass of O) + (2 * atomic mass of H)
= 55.85 g/mol + (2 * 16.00 g/mol) + (2 * 1.01 g/mol)
= 55.85 g/mol + 32.00 g/mol + 2.02 g/mol
= 89.87 g/mol
Grams of Fe(OH)2 = moles of Fe(OH)2 * molar mass of Fe(OH)2
= 4 moles * 89.87 g/mol
= 359.48 g
Therefore, 359.48 grams of Fe(OH)2 would be formed.
To find the number of grams of Fe(OH)2 formed, we need to use stoichiometry, which is a way to relate the amounts of reactants and products in a chemical reaction.
First, we should calculate the number of moles of FeCl2 used. The molar mass of FeCl2 is the sum of the atomic masses of iron (Fe) and chlorine (Cl), which is approximately 55.85 g/mol + (2 × 35.45 g/mol) = 126.75 g/mol.
To convert grams to moles, we divide the given mass by the molar mass:
Number of moles of FeCl2 = 507 g / 126.75 g/mol = 4 moles of FeCl2.
Next, we need to determine the stoichiometric ratio between FeCl2 and Fe(OH)2 in the balanced equation. From the equation, we see that 1 mole of FeCl2 reacts to form 1 mole of Fe(OH)2. This means that the ratio of Fe(OH)2 to FeCl2 is 1:1.
Since we have 4 moles of FeCl2, we can conclude that 4 moles of Fe(OH)2 will be formed.
Finally, we calculate the mass of Fe(OH)2. The molar mass of Fe(OH)2 is the sum of the atomic masses of iron (Fe), oxygen (O), and hydrogen (H). It is approximately 55.85 g/mol + (2 × 16.00 g/mol) + (2 × 1.01 g/mol) = 89.91 g/mol.
To convert moles to grams, we multiply the number of moles by the molar mass:
Mass of Fe(OH)2 = 4 moles × 89.91 g/mol = 359.64 g.
Therefore, approximately 359.64 grams of Fe(OH)2 would be formed.