Asked by Jeremy
Hi, I posted my question earlier but I was having some difficulty with it.
2Al+ 3Cl2-->2AlCl3
You are given 31.0g of aluminum and 36.0g of chlorine gas.
1.If you had excess chlorine, how many moles of aluminum chloride could be produced from 31.0g of aluminum?
_________________________________________
This is my work so far:
Cl2-36.0g/70.9= 0.507mol
Al-31.0g/26.98=1.15mol
Therefore Chlorine is the limiting reagent, since I have less that 3/2.
Cl2:AlCl3= 3:2
0.507mol (3/2)=0.76 mol AlCl3.
Please check my answer and significant figures. I am pretty sure I messed up!
2Al+ 3Cl2-->2AlCl3
You are given 31.0g of aluminum and 36.0g of chlorine gas.
1.If you had excess chlorine, how many moles of aluminum chloride could be produced from 31.0g of aluminum?
_________________________________________
This is my work so far:
Cl2-36.0g/70.9= 0.507mol
Al-31.0g/26.98=1.15mol
Therefore Chlorine is the limiting reagent, since I have less that 3/2.
Cl2:AlCl3= 3:2
0.507mol (3/2)=0.76 mol AlCl3.
Please check my answer and significant figures. I am pretty sure I messed up!
Answers
Answered by
DrBob222
Yes, you did.
The first part is not a limiting reagent since you have all of the Cl2 needed.
moles Al = 31.0/26.98 = 1.149
moles AlCl3 = 1.149 moles Al x (2 moles AlCl3/2 moles Al) = 1.149 x (1/1) = 1.149 moles AlCl3 which rounds to 1.15 to three s.f.
#2a You can do it two ways. The way I suggested, since you had to do #1 anyway, is to keep #1 in mind and work #1 with 36.0 g Cl2 and all the Al needed.
moles Cl2 in 36.0 g is
36.0/70.9 = 0.50776 (which I would have rounded to 0.508 BUT I usually carry extra places(in the calculator) and round at the end of the problem.
moles AlCl3 = 0.50776 mols Cl2 x (2 moles AlCl3/3 moles Cl2) = 0.3385 moles which rounds to 0.338 moles AlCl3. (Your error is in the conversion factor.) Then I compare moles from #1 where we had all of the Cl2 needed (1.15) with #2 where we had all of the Al we needed (0.338) and the correct value is the smaller of the two; that is 0.338 moles AlCl3 formed.
2b. The other way Bob Pursley showed you is the way you did it to determine Cl2 was the limiting reagent.
31.0/26.98 = 1.15 moles Al and
(31.0/26.98) x (3 moles Cl2/2 moles Al) = 1.72 moles Cl2 needed and we don't have that much.
(36.0/70.9 = 0.508 moles Cl2.
(36.0/70.9) x (2 moles Al/3 moles Cl2) = 0.338 moles Al needed and we have that much; therefore, your work is ok in determining the limiting reagent.
The first part is not a limiting reagent since you have all of the Cl2 needed.
moles Al = 31.0/26.98 = 1.149
moles AlCl3 = 1.149 moles Al x (2 moles AlCl3/2 moles Al) = 1.149 x (1/1) = 1.149 moles AlCl3 which rounds to 1.15 to three s.f.
#2a You can do it two ways. The way I suggested, since you had to do #1 anyway, is to keep #1 in mind and work #1 with 36.0 g Cl2 and all the Al needed.
moles Cl2 in 36.0 g is
36.0/70.9 = 0.50776 (which I would have rounded to 0.508 BUT I usually carry extra places(in the calculator) and round at the end of the problem.
moles AlCl3 = 0.50776 mols Cl2 x (2 moles AlCl3/3 moles Cl2) = 0.3385 moles which rounds to 0.338 moles AlCl3. (Your error is in the conversion factor.) Then I compare moles from #1 where we had all of the Cl2 needed (1.15) with #2 where we had all of the Al we needed (0.338) and the correct value is the smaller of the two; that is 0.338 moles AlCl3 formed.
2b. The other way Bob Pursley showed you is the way you did it to determine Cl2 was the limiting reagent.
31.0/26.98 = 1.15 moles Al and
(31.0/26.98) x (3 moles Cl2/2 moles Al) = 1.72 moles Cl2 needed and we don't have that much.
(36.0/70.9 = 0.508 moles Cl2.
(36.0/70.9) x (2 moles Al/3 moles Cl2) = 0.338 moles Al needed and we have that much; therefore, your work is ok in determining the limiting reagent.
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