For the reaction 4FeCl2(aq) + 3O2(g) - 2Fe2O3(s) + 4Cl2(g); how many grams of FeO3 are produced from 8.71 x 10 to the 21st power molecules of O2?? Help Please!
4FeCl2(aq) + 3O2(g) - 2Fe2O3(s) + 4Cl2(g)
mols O2 = 8.71E21 molecules x (1 mol/6.02E23 molecules) = ?
Using the coefficients in the balanced equation, convert mols O2 to mols Fe2O3
Then convert mols Fe2O3 to g Fe2O3 with g = mol Fe2O3 x molar mass Fe2O3.
To determine the number of grams of Fe2O3 produced from a given number of molecules of O2, you need to follow these steps:
Step 1: Convert the given number of molecules of O2 to moles.
To do this, use Avogadro's number (6.022 x 10^23) to convert from molecules to moles.
Given: 8.71 x 10^21 molecules of O2
Conversion: (8.71 x 10^21 molecules) / (6.022 x 10^23 molecules/mol) = x mol
Step 2: Use the balanced chemical equation to determine the mole ratio between O2 and Fe2O3.
From the balanced equation, we know that 3 moles of O2 react to form 2 moles of Fe2O3.
Step 3: Calculate the moles of Fe2O3 produced.
Multiply the moles of O2 from step 1 by the mole ratio determined in step 2.
Moles of Fe2O3 = (x mol O2) * (2 mol Fe2O3 / 3 mol O2) = y mol
Step 4: Convert moles of Fe2O3 to grams.
To do this, use the molar mass of Fe2O3. The molar mass of Fe2O3 can be found by adding the atomic masses of the elements: 2 moles of Fe (55.845 g/mol) and 3 moles of O (16.00 g/mol).
Molar mass of Fe2O3 = (2 * 55.845 g/mol) + (3 * 16.00 g/mol) = z g/mol
Grams of Fe2O3 = (y mol Fe2O3) * (z g Fe2O3 / 1 mol Fe2O3) = Answer
By following these steps, you can calculate the number of grams of Fe2O3 produced from a given number of molecules of O2.