Dr. Bob222 Please don't get frustrated with me, I'm really trying to figure this out... UGH!!

Question

I'm starting over again... Please advise...
. Consider the following chemical equation:
TiCl4(g) + 2Mg(l) → Ti(s) + 2MgCl2(l)
3.54×107g of TiCl4(g) were reacted completely and 7.91×106g of Ti(s) was obtained in the experiment.
a. (10 points) Calculate the theoretical yield of Ti(s).
In order to find TY I have to find the limiting agent.. ?? ugh.. Ok, Ti=47.88 Cl4=35.45*4... To find moles in TiCl4 I take 3.54*10^7 * 1moleTiCl4/189.68 = 184,521.89 moles? But I need TY of Ti?? 7.91*10^6 * 1mole Ti/47.88=165,204.68 moles Ti???? I'm completely lost.. I guess I don't even know how to correctly find the moles of things?? I'm taking this class online at UTA with no help from a teacher and I'm trying to teach myself.. and I'm struggling so bad!!!! I think after your help I am doing it right then I confuse myself again..

b. (5 points) What is the actual yield of Ti(s) in this experiment? 7.91*10^6 it's given...

c. (10 points) Calculate the % yield of Ti(s) in this experiment. Percent yield is AY/TY so would it be?? 7.91*10^6/165,204.68?? the moles of Ti? or is that the TY of Ti? I'm so confused.. You said before you got the TY to be 8.9E6? how??

Answer 1

3.54 x 10^7 g TiCl4 x (1 mol/189.68 g) x (1 mol Ti/1 mol TiCl4) x (47.88 g/1 mol) = 8.94 x 10^6 g Ti

Answer 2

Percent yield is equal to the actual amount yield divided by the theoretical amount, so: 7.91 x 10^6 all divided by 8.94 x 10^6 = 88.5% yield

Is this right???