If 3.0 moles of HCl are consumed in the reaction below, how many moles of FeCl3 are produced?
6HCl + Fe2O3 --> 2FeCl3 + 3H2O
Here is a solved example of a
stoichiometry problem. Just follow the steps.
http://www.jiskha.com/science/chemistry/stoichiometry.html
Post your work if you get stuck.
To determine the number of moles of FeCl3 produced, we need to use the mole ratio between HCl and FeCl3 from the balanced equation.
From the balanced equation:
6 moles of HCl react to produce 2 moles of FeCl3.
So, if 6 moles of HCl react, we can set up a proportion to find how many moles of FeCl3 are produced by 3.0 moles of HCl:
6 moles HCl 2 moles FeCl3
------------------- = --------------------
3.0 moles HCl x moles FeCl3
Cross-multiplying the equation, we get:
6 moles HCl * x moles FeCl3 = 3.0 moles HCl * 2 moles FeCl3
Rearranging the equation to solve for x, we have:
x moles FeCl3 = (3.0 moles HCl * 2 moles FeCl3) / 6 moles HCl
x moles FeCl3 = 1.0 moles FeCl3
Therefore, if 3.0 moles of HCl are consumed in the reaction, 1.0 mole of FeCl3 is produced.
To determine the number of moles of FeCl3 produced, we need to use stoichiometry, which is the ratio of moles between the reactants and the products.
From the balanced chemical equation:
6HCl + Fe2O3 -> 2FeCl3 + 3H2O
We can see that the ratio between HCl and FeCl3 is 6:2 or 3:1. This means that for every 6 moles of HCl consumed, 2 moles of FeCl3 are produced.
Therefore, to find the number of moles of FeCl3 produced when 3.0 moles of HCl are consumed, we can set up a proportion:
(3.0 moles HCl / 6 moles HCl) = (x moles FeCl3 / 2 moles FeCl3)
Cross-multiplying gives us:
6 * x = 3.0 * 2
Simplifying the equation:
6x = 6.0
Solving for x, we get:
x = 1.0
So, when 3.0 moles of HCl are consumed, 1.0 mole of FeCl3 is produced.