Question

What is the theoretical yield of aluminum oxide if 1.60mol of aluminum metal is exposed to 1.50mol of oxygen?

Answer 1

First write down the reaction equation

Answer 2

4Al+3O2→2Al2O3

Answer 3

That's right.
Now the ratio of mol aluminium metal : aluminium oxide is 4:2
So 4 moles of aluminium are used to produce 2 moles of aluminium oxide.

The ratio of mol aluminum metal : oxygen is 4:3
So for using 4 moles aluminium, we need 3 mol oxygen.

We have 1.6 mol aluminium metal and 1.5 mol oxygen
how many moles of oxygen do we need to let all the aluminium metal react?

Answer 4

no.
use the ratio.
Al:O2 = 4:3
so when Al is 1.6, them O2 is 1.6 times 3 divided by 4 which is 1.2 mol oxygen

Answer 5

okay so it is 1.2

Answer 6

the solution won't help you.
In a test I won't be there to hand you over the answers...

calculating how many moles O2 you need is just to check if O2 is in excess. We need 1.2 mol and we have 1.5 mol, which means that O2 is in excess and Al is the limiting reactant.

The limiting reactant is the reactant which will be used up entirely in the reaction.

Now we need the Al:Al2O3 ratio, which is 4:2
we have 1.6 mol Al, how many moles of Al2O3 will we get?

Answer 7

no

Answer 8

4 = 2
1.6 = ?

you can see that 2 is half of 4
so what's half of 1.6?

Answer 9

0.8

Answer 10

yes

Answer 11

0.8 mol Al2O3 is produceed when 1.6 mol Al reacts with 1.2 mol O2

Answer 12

In Part A, we saw that the theoretical yield of aluminum oxide is 0.800mol . Calculate the percent yield if the actual yield of aluminum oxide is 0.416mol .

Answer 13

what is the equation

Answer 14

is it percent yield=actual / theoritical

Answer 15

i got 52 %

Answer 16

right

Answer 17

thanks i got it

Answer 18

canyou help me withsome more so i get a good feeling abou this chemistry

Answer 19

Yea sorry I was looking at something else

Answer 20

i will post it above