Asked by Jennie

Someone please tell me if I'm doing this right... It's due tonight!!

Dr. Bob222, Yesterday I posted a question and you answered me with how to calculate it.. Can you tell me if I'm doing this correctly?? Please!
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. Calculate the theoretical yield of Ti(s).
Ok, The atomic weight of Ti=47.88 Cl=35.45 (*4) Mg=24.31 (*2)
Total Molar Mass of TiCl4=189.68g/mol
to calculate TY of Ti = 47.88/189.68= 0.252 moles of Ti??? Where you wrote TiCl4 * (1mol Ti/1mol TiCl4) am I supposed to multiply 189.68 *0.252?? if so that would = 47.80 ??? Or just 0.252 moles is the answer? And the TY yield is 0.252 moles Ti * Ti atomic weight? 47.88= 12.07g??? is this right?

b.What is the actual yield of Ti(s) in this experiment? AY =OHH this is given already, as 7.91*10E6 ok..

c.Calculate the % yield of Ti(s) in this experiment. AY/TY *100 which would be 7.91*10E6/??? I can't figure out the correct theoretical yield.. I think I'm confusing myself... Help!!
ok, so the TY is moles of Ti (0.252) * atomic mass of Ti (47.88) which = 12.07g TY of Ti. So to calculate the percent yield, it's (7.91*10E6/12.07)*100? = 65,534,382.76 do I put that in scientific notation? what is that 6.55 * 10E-7???

Please help on this?? tell me if I'm on the right track?? Thank you so much for your help!
Answered by DrBob222
See my response above.
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