Question

3.0 mol of aluminum is mixed with 5.3 mol of cl2
2Al(s) + 3Cl2(g) --->2AlCl3(s)
a) identify the limiting reagent
b) calculate the number of moles of product formed
c) calculate the number of moles of excess reagent remaining after the reaction

Answer 1

http://chemhnhs.com/ChemHNHS%20Website/PC%20Chap12/Pearson_Resources12/nachemte_12sgas.pdf

Answer 2

this might help idk if i can sorry

Answer 3

You are given moles of aluminum and moles of cl2. Convert those into grams and then do two separate stoichiometry problems to figure out the limiting reagent. The smaller number is the right answer.
If you need an explanation I could kind of help.

Answer 4

I get the convert into moles but that's when I get lost

Answer 5

You mean convert the moles into grams? or the entire stoichiometry process?

Answer 6

Ok, I know how to go from moles to grams, but that's when I get lost and don't know what to do

Answer 7

We need to find which is limiting, If we were to compare amount of Al in moles with Cl2
\[3molAl \times \frac{3molCl_2}{2molAl}=4.5molCl_2\]
3mol of Al gives 4.5 mol Cl2, but originally u have 5.3 mol of Cl2, so Al will be limiting here

Answer 8

But remember the smaller amount of a reactant isn't always the limiting reactant!

Answer 9

Since its mole ratio between Al and product is same, then 4.5 mol of AlCl3 formed

Answer 10

Balance the chemical equation.
What did they ask you to find? Write the grams of this “asked for” compound on the far right.
What did they give you to start with? Write the grams of this “given” compound on the far left.
Write the grams of the “given” compound in the denominator of the next factor. Write only the word grams. Do not write the number from the previous factor.
Write the moles of “given” in the numerator of the same factor.
Place the appropriate numbers with the correct units. (The mole will always be a 1, and the grams will always have the atomic or molecular weight from the periodic chart in this step.)
Place the moles of “given” in the denominator of the next factor.
Place the moles of “asked for” in the numerator of the same factor.
Place the coefficients from the balanced equation in the factor in the appropriate place.
Place the moles of “asked for” in the denominator of the next factor.
Place the grams of “asked for” in the numerator of the same factor.
Place the appropriate numbers next to the correct units. (The mole will always be a 1, and the grams will always have the atomic or molecular weight from the periodic chart in this step.)

Sorry. Here are the steps for a stoichiometry problem. Do two separate problems: one starting with Al and one with Cl2 and pick the smallest answer.
Kind of long and maybe confusing at first but take it slow and you'll eventually get it.