If 507 g FeCl2 were used up in the reaction FeCl2 + 2NaOH Fe(OH)2(s) + 2NaCl, how many grams of NaCl would be made?
To find out how many grams of NaCl would be made, we need to calculate the stoichiometric ratio between FeCl2 and NaCl in the balanced equation.
The balanced equation is:
FeCl2 + 2NaOH -> Fe(OH)2(s) + 2NaCl
From the balanced equation, we see that 1 mole of FeCl2 reacts with 2 moles of NaCl.
To calculate the number of moles of FeCl2, we can use the formula:
moles = mass / molar mass
The molar mass of FeCl2 is 55.85 g/mol + 2(35.45 g/mol) = 126.75 g/mol.
So, the number of moles of FeCl2 used can be calculated as:
moles of FeCl2 = 507 g / 126.75 g/mol ~= 4 moles
Since the stoichiometric ratio is 1:2 between FeCl2 and NaCl, the number of moles of NaCl produced will be twice the number of moles of FeCl2 used. Therefore, the number of moles of NaCl produced is:
moles of NaCl = 4 moles x 2 = 8 moles
Now we can calculate the mass of NaCl produced using the formula:
mass = moles x molar mass
The molar mass of NaCl is 22.99 g/mol + 35.45 g/mol = 58.44 g/mol.
So, the mass of NaCl produced is:
mass of NaCl = 8 moles x 58.44 g/mol = 467.52 g
Therefore, approximately 467.52 grams of NaCl would be made in this reaction.
To find out how many grams of NaCl would be made, we need to determine the molar ratio between FeCl2 and NaCl in the balanced chemical equation.
First, we need to determine the molar mass of FeCl2. The molar mass of Fe is 55.85 g/mol, and the molar mass of Cl is 35.45 g/mol. Therefore, the molar mass of FeCl2 is calculated as follows:
Molar mass of FeCl2 = (1 * molar mass of Fe) + (2 * molar mass of Cl)
= (1 * 55.85 g/mol) + (2 * 35.45 g/mol)
= 55.85 g/mol + 70.90 g/mol
= 126.75 g/mol
Next, we need to determine the molar ratio between FeCl2 and NaCl in the balanced chemical equation:
FeCl2 + 2NaOH Fe(OH)2(s) + 2NaCl
From the equation, we can see that the ratio of FeCl2 to NaCl is 1:2. This means that for every 1 mole of FeCl2, 2 moles of NaCl are produced.
Now, we can calculate the number of moles of FeCl2 used in the reaction:
Number of moles of FeCl2 = mass of FeCl2 / molar mass of FeCl2
= 507 g / 126.75 g/mol
= 4 moles
Since the molar ratio between FeCl2 and NaCl is 1:2, we can calculate the number of moles of NaCl produced:
Number of moles of NaCl = 2 moles of NaCl / 1 mole of FeCl2 * 4 moles of FeCl2
= 2 * 4
= 8 moles
Finally, we can calculate the mass of NaCl produced using the number of moles of NaCl and its molar mass:
Mass of NaCl = number of moles of NaCl * molar mass of NaCl
= 8 moles * (22.99 g/mol + 35.45 g/mol)
= 8 moles * 58.44 g/mol
= 467.52 g
Therefore, if 507 g of FeCl2 were used up in the reaction, approximately 467.52 g of NaCl would be produced.
Write the equation and balance it.
Convert 507 g FeCl2 to mols. mols = grams/molar mass.
Using the coefficients in the balanced equation convert mols FeCl2 to mols NaCl.
Now convert mols NaCl to g. g = mols x molar mass.