would 0.360 mol of hydrochloric acid be sufficient to react with 10.0 g ferric oxide?
To determine whether 0.360 mol of hydrochloric acid is sufficient to react with 10.0 g of ferric oxide, we need to use stoichiometry and balanced chemical equation.
First, let's write the balanced chemical equation for the reaction between hydrochloric acid (HCl) and ferric oxide (Fe2O3):
Fe2O3 + 6HCl -> 2FeCl3 + 3H2O
From the balanced equation, we can see that it takes 6 moles of hydrochloric acid to react with 1 mole of ferric oxide.
To find the molar amount of ferric oxide in 10.0 g, we need to calculate its moles. We can use the molar mass of ferric oxide to convert the grams to moles.
Molar mass of Fe2O3 = 2(55.845 g/mol) + 3(16.00 g/mol) = 159.69 g/mol
Moles of Fe2O3 = mass / molar mass = 10.0 g / 159.69 g/mol ≈ 0.063 mol
Now, we can compare the mol ratio between HCl and Fe2O3.
For every 6 moles of HCl, we need 1 mole of Fe2O3. Therefore, we need to multiply the moles of Fe2O3 by the ratio:
0.063 mol Fe2O3 * (6 mol HCl / 1 mol Fe2O3) = 0.378 mol HCl
Based on the stoichiometry, we need 0.378 mol of hydrochloric acid to react with 10.0 g of ferric oxide. Since you have 0.360 mol of hydrochloric acid, it is not sufficient to react completely with the given amount of ferric oxide.