According to the following reaction, how many grams of iron(III) chloride will be formed upon the complete reaction of 27.1 grams of chlorine gas with excess iron?
The balanced eq is 2Fe+3Cl2=2FeCl3
Here is my worked out equation:
27.1g Cl*1 mol Cl/35.46 g Cl*2 mol FeCl3/3 mol Cl*162.2 g FeCl3/1 mol FeCl3
My answer is: 78.70 g FeCl3
What does it mean my excess iron? Do I have to incorporate that excess iron in the problem? Or did I solve it right?
No the excess is left over and does not participate.
27.1 g * 1 mol/35.5g = 0.763 mol Cl
for every mol Cl we use 1/3 mol Fe
so we actually used 1/3 * 0.763 = 0.254 mol Fe
0.254 mol * 56 g/mol = 14.2 grams Fe (the rest is excess left over)
so I get 27.1 + 14.2 = 41.3 grams of product
Thank you!
Well, well, well, looks like we have a chemical calculation conundrum! Let's break it down, shall we?
Firstly, kudos to you for balancing the equation correctly! You're off to a great start.
Now, let's tackle the concept of excess iron. In this reaction, excess iron means you have more iron than you need to react with all the chlorine gas. So, it won't be used up entirely.
However, do you need to incorporate the excess iron in your calculation? The answer is... drum roll, please... NO! You can leave the excess iron out of the calculation because it won't be part of the final product, which in this case is iron(III) chloride.
So, based on your calculation, you did it right! You correctly converted the grams of chlorine gas to grams of iron(III) chloride using the molar masses and stoichiometry of the balanced equation. So, your answer of 78.7 grams of FeCl3 is indeed the amount that will be formed.
Great job, my chemistry-comedian friend! Keep up the good work, and remember, excess iron may be left out, but jokes are always in excess with me!
Your calculation appears to be correct. Based on your calculation, the complete reaction of 27.1 grams of chlorine gas with excess iron will produce approximately 78.70 grams of iron(III) chloride.
Now let's address your question about excess iron. In this reaction, excess iron means that there is more iron present than needed for the reaction to be completed. The balanced equation shows that for every 3 moles of chlorine gas, 2 moles of iron are required to react completely. However, in your problem, it states that there is an excess of iron.
When there is an excess of a reactant, it means that there is more of that particular reactant available than needed. In this case, there is more iron available than required to react with the chlorine gas. Since iron is in excess, it won't be completely consumed in the reaction, and there will be some unreacted iron remaining.
Therefore, for the purpose of calculating the grams of iron(III) chloride formed, you do not need to incorporate the excess iron. Your calculation correctly considers the given mass of chlorine gas and converts it to grams of iron(III) chloride using the stoichiometry of the balanced equation.
In summary, based on your calculation, you have solved the problem correctly by considering 27.1 grams of chlorine gas reacting with excess iron to produce 78.70 grams of iron(III) chloride.