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!
Partly on the right track and partly not.
. 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 ok to here
to calculate TY of Ti = 47.88/189.68= 0.252 moles of Ti???
No. mols = grams/molar mass. The problem gives grams TiCl4 = 3.54E7 grams. So mols = 3.54E7/189.68 = ?. You used the atomic mass of Ti, not the mass TiCl4 given in the problem. Where you wrote TiCl4 * (1mol Ti/1mol TiCl4) am I supposed to multiply 189.68 *0.252?? That was to convert mols TiCl4 (which you started with) to mols Ti (which you produced). That is mols TiCl4 from the previous step x (1 mol Ti/1 mol TiCl4) = mols TiCl4 x 1/1 = just mols TiCl4 and that = mols Ti produced. 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? Then you convert mols Ti produced to g Ti produced by g Ti = mols Ti x atomic mass Ti = grams Ti. That is the theoretical yield.
b.What is the actual yield of Ti(s) in this experiment? AY =OHH this is given already, as 7.91*10E6 ok..
Yes, the actual yield is 7.91E6 grams. That is given in the problem
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???
I think after you plug in the actual yield and the theoretical yield you will get % yield ok. I ran through the theoretical yield quickly and got approximately about 8.9E6 grams for TY but you should confirm that and take it to at least one more place. That 6.55E-7 (which is 6.55E7 if you put it CORRECTLY in scientific notation is the answer for % yield EXCEPT you didn't calculate TY right since 0.252 is not the mols Ti and that is because you didn't calculate mols TiCl4 right. I think this should clear up some of the steps.
To determine if you are on the right track with your calculations, let's break down each step and check them one by one:
a) Calculate the theoretical yield of Ti(s):
You correctly identified the molar mass of TiCl4 as 189.68 g/mol. To calculate the theoretical yield, you need to convert the mass of TiCl4 (3.54×10^7 g) to moles by dividing it by the molar mass:
3.54×10^7 g TiCl4 * (1 mol TiCl4 / 189.68 g TiCl4) ≈ 186,629.41 mol TiCl4
Now, you multiply the moles of TiCl4 by the stoichiometric coefficient of Ti (1 mol Ti / 1 mol TiCl4) to find the moles of Ti:
186,629.41 mol TiCl4 * (1 mol Ti / 1 mol TiCl4) ≈ 186,629.41 mol Ti
Finally, you multiply the moles of Ti by the atomic weight of Ti (47.88 g/mol) to find the theoretical yield:
186,629.41 mol Ti * 47.88 g Ti/mol ≈ 8,931,437.72 g Ti
So the theoretical yield of Ti(s) is approximately 8,931,437.72 g.
b) The actual yield of Ti(s) is given as 7.91×10^6 g, so you correctly identified this number.
c) To calculate the percent yield, you divide the actual yield (AY) by the theoretical yield (TY) and multiply by 100:
Percent Yield = (AY / TY) * 100
Plugging in the values:
Percent Yield = (7.91×10^6 g / 8,931,437.72 g) * 100 ≈ 0.08853%
To convert this to scientific notation, you can express it as 8.853×10^-4%.
Overall, it appears that you are on the right track with your calculations. Just make sure to double-check your conversions and units to avoid any errors. Good luck with your assignment!