What is the limiting reagent for 6HCl + Fe2O3 = 2FeCl3 + 3H2O ? 6HCl has 18.44 moles and Fe2O3 has 2.91 moles. Also how many moles would FeCl3 produce?
To determine the limiting reagent, we need to compare the number of moles of each reactant to the stoichiometric ratio given by the balanced equation.
Let's start by calculating the moles of FeCl3 that can be formed from each reactant:
From the balanced equation:
6HCl + Fe2O3 -> 2FeCl3 + 3H2O
According to the stoichiometry, 6 moles of HCl react with 1 mole of Fe2O3 to produce 2 moles of FeCl3. Thus, we can set up the following ratio:
6HCl : 1Fe2O3 : 2FeCl3
Now, let's calculate the moles of FeCl3 that can be produced using the given information:
Moles of FeCl3 from HCl = (18.44 moles HCl) x (2 moles FeCl3 / 6 moles HCl) = 6.147 moles FeCl3
Moles of FeCl3 from Fe2O3 = (2.91 moles Fe2O3) x (2 moles FeCl3 / 1 mole Fe2O3) = 5.82 moles FeCl3
So, the limiting reagent is the reactant that produces the fewer moles of the desired product. In this case, Fe2O3 produces 5.82 moles of FeCl3, which is fewer than the 6.147 moles produced by HCl. Therefore, Fe2O3 is the limiting reagent.
Next, let's calculate the moles of FeCl3 that can be produced using the limiting reagent:
We have determined that Fe2O3 is the limiting reagent, so we will use its moles to calculate the moles of FeCl3 produced.
Using the stoichiometry from the balanced equation:
1 mole of Fe2O3 produces 2 moles of FeCl3
Moles of FeCl3 = (2.91 moles Fe2O3) x (2 moles FeCl3 / 1 mole Fe2O3) = 5.82 moles FeCl3
Therefore, 5.82 moles of FeCl3 can be produced from the given amount of reactants.
To determine the limiting reagent, we need to compare the moles of each reactant to the stoichiometric ratio of the balanced equation.
The balanced equation is: 6HCl + Fe2O3 = 2FeCl3 + 3H2O
From the given information:
- 6HCl has 18.44 moles
- Fe2O3 has 2.91 moles
We can use the stoichiometric ratio of the balanced equation to find out how many moles of FeCl3 can be produced.
From the balanced equation, we see that the ratio between HCl and FeCl3 is 6:2, meaning that 6 moles of HCl react with 2 moles of FeCl3. Therefore, for every 6 moles of HCl, we would expect to get 2 moles of FeCl3.
However, we also need to consider the stoichiometric ratio between Fe2O3 and FeCl3. From the balanced equation, we can see that the ratio between Fe2O3 and FeCl3 is 1:2, meaning that 1 mole of Fe2O3 reacts with 2 moles of FeCl3.
To determine the limiting reagent, we need to compare the moles of both reactants to see which one is less.
For HCl:
18.44 moles HCl * (2 moles FeCl3 / 6 moles HCl) = 6.1467 moles FeCl3
For Fe2O3:
2.91 moles Fe2O3 * (2 moles FeCl3 / 1 mole Fe2O3) = 5.82 moles FeCl3
From the calculations, we can see that the moles of FeCl3 produced from 6HCl is 6.1467 moles, while the moles of FeCl3 produced from Fe2O3 is 5.82 moles.
Therefore, the limiting reagent is Fe2O3, as it produces fewer moles of FeCl3.
To answer the second part of your question, if Fe2O3 is the limiting reagent, it will produce 5.82 moles of FeCl3.