Consider this reaction:FeCl2 + 2NaOH Fe(OH)2(s) + 2NaClIf 507 g FeCl2 were used up in the reaction, how many grams of NaCl would be made?A.1014 g NaClB.467.52 g NaClC.233.76 g NaClD.649.05 g NaClSUBMITarrow_backPREVIOUS

To solve this problem, we need to use stoichiometry, which is a method in chemistry that makes use of the relationship between reactants and products in a balanced chemical equation.

Step 1: Write down the balanced chemical equation: FeCl2 + 2NaOH → Fe(OH)2 + 2NaCl

Step 2: Determine the molar mass of FeCl2 and NaCl. You can find these values on a periodic table. The molar mass of FeCl2 is approximately 126.75 g/mol and the molar mass of NaCl is approximately 58.44 g/mol.

Step 3: Calculate the number of moles of FeCl2 used in the reaction. This is done by dividing the mass of FeCl2 given in the problem (507 g) by its molar mass. 507 g FeCl2 * (1 mol FeCl2 / 126.75 g FeCl2) = 4 moles FeCl2

Step 4: Use the stoichiometric ratio from the balanced chemical equation to find the number of moles of NaCl produced. From the balanced equation, we can see that 2 moles of NaCl are produced for every 1 mole of FeCl2 used. 4 moles FeCl2 * (2 moles NaCl / 1 mole FeCl2) = 8 moles NaCl

Step 5: Convert the number of moles of NaCl to grams using its molar mass. 8 moles NaCl * (58.44 g NaCl / 1 mole NaCl) = 467.52 g NaCl

So, the answer is B. 467.52 g NaCl.