stoichiometry problem
Fe2O3+HCl=H2O+FeCl3
If 42.2 grams of iron(III) Oxide react with HCl how many gramd of iron(III)chloride should be produced
Balance the equation first.
Fe2O3 + 6HCl = 3H2O + 2FeCl3
mols Fe2O3 = grams/molar mass = ?
Using the coefficients in the balanced equation, convert mols Fe2O3 to mols FeCl3.
Now convert mols FeCl3 to grams.
grams FeCl3 = mols FeCl3 x molar mass FeCl3.
To solve this stoichiometry problem, we need to use the balanced chemical equation and the molar masses of the compounds involved.
First, let's write down the balanced chemical equation for the reaction:
Fe2O3 + 6HCl → 3H2O + 2FeCl3
The equation tells us that 1 mole of Fe2O3 reacts with 6 moles of HCl to produce 2 moles of FeCl3.
Now, we can follow these steps to calculate the grams of FeCl3 produced:
Step 1: Calculate the number of moles of Fe2O3.
Given mass of Fe2O3 = 42.2 grams
Molar mass of Fe2O3 = 55.85 g/mol (2 atoms of Fe with molar mass 55.85 g/mol + 3 atoms of O with molar mass 16.00 g/mol)
Number of moles of Fe2O3 = given mass / molar mass
= 42.2 g / 55.85 g/mol
Step 2: Convert the moles of Fe2O3 to moles of FeCl3 using the stoichiometry of the balanced equation.
Using the ratio from the balanced equation, 2 moles of FeCl3 are produced from 1 mole of Fe2O3.
Number of moles of FeCl3 = Number of moles of Fe2O3 * (2 moles FeCl3 / 1 mole Fe2O3)
Step 3: Calculate the grams of FeCl3 produced.
Given mass of FeCl3 = ?
Molar mass of FeCl3 = 162.20 g/mol (2 atoms of Fe with molar mass 55.85 g/mol + 3 atoms of Cl with molar mass 35.453 g/mol)
Grams of FeCl3 = Number of moles of FeCl3 * Molar mass of FeCl3
Now, let's calculate the grams of FeCl3 produced:
Number of moles of Fe2O3 = 42.2 g / 55.85 g/mol = 0.755 moles
Number of moles of FeCl3 = 0.755 moles * (2 moles FeCl3 / 1 mole Fe2O3) = 1.51 moles
Grams of FeCl3 = 1.51 moles * 162.20 g/mol ≈ 244.59 grams
Therefore, approximately 244.59 grams of FeCl3 should be produced when 42.2 grams of iron(III) oxide reacts with HCl.
To solve this stoichiometry problem, you need to follow a few steps:
Step 1: Write and balance the chemical equation
The given chemical equation is already balanced.
Step 2: Convert the given mass of the reactant to moles
You have 42.2 grams of iron(III) oxide (Fe2O3). To convert this mass to moles, you need to divide it by the molar mass of iron(III) oxide.
Molar mass of Fe2O3:
Fe: 2 atoms x atomic mass of Fe = 2 x 55.85 g/mol
O: 3 atoms x atomic mass of O = 3 x 16.00 g/mol
Total molar mass = 2 x 55.85 + 3 x 16.00 = 159.69 g/mol
Number of moles of Fe2O3 = Mass of Fe2O3 / Molar mass of Fe2O3
Number of moles of Fe2O3 = 42.2 g / 159.69 g/mol = 0.264 mol
Step 3: Determine the mole ratio between the reactant and the product
By examining the balanced chemical equation, you can see that the mole ratio between Fe2O3 and FeCl3 is 1:1. This means that for every 1 mole of Fe2O3, you will produce 1 mole of FeCl3.
Step 4: Calculate the moles of FeCl3 formed
Since the mole ratio of Fe2O3 to FeCl3 is 1:1, the number of moles of FeCl3 formed will be equal to the number of moles of Fe2O3.
Number of moles of FeCl3 formed = Number of moles of Fe2O3 = 0.264 mol
Step 5: Convert moles of FeCl3 to grams
To calculate the mass of FeCl3 formed, you need to multiply the number of moles of FeCl3 by its molar mass.
The molar mass of FeCl3 can be obtained by summing the atomic masses of each element:
Fe: 1 atom x atomic mass of Fe = 1 x 55.85 g/mol
Cl: 3 atoms x atomic mass of Cl = 3 x 35.45 g/mol
Total molar mass = 55.85 + 3 x 35.45 = 162.20 g/mol
Mass of FeCl3 formed = Number of moles of FeCl3 x Molar mass of FeCl3
Mass of FeCl3 formed = 0.264 mol x 162.20 g/mol = 43.00 grams
Therefore, 42.2 grams of iron(III) oxide will react to produce 43.00 grams of iron(III) chloride.