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!
See my response above.
Based on the information you provided, let's go step by step to check if you're doing the calculations correctly.
a. The theoretical yield (TY) of Ti(s) can be calculated using the stoichiometry of the balanced chemical equation. According to the equation:
1 mole of TiCl4 reacts to produce 1 mole of Ti(s).
You correctly calculated the molar mass of TiCl4 as 189.68 g/mol. Then, to find the theoretical yield of Ti(s), you need to multiply the number of moles of TiCl4 (0.252 moles) by the molar mass of Ti (47.88 g/mol).
So, the correct calculation is: TY = 0.252 moles of Ti * 47.88 g/mol = 12.07 g of Ti.
Therefore, your calculation for the theoretical yield is correct.
b. The actual yield (AY) of Ti(s) is given as 7.91×10^6 g. You mentioned that this value is already given, so you don't need to calculate it.
c. The percent yield can be calculated by dividing the actual yield (AY) by the theoretical yield (TY), and then multiplying by 100.
The correct calculation is: % yield = (AY / TY) * 100 = (7.91×10^6 g / 12.07 g) * 100 = 6.55 * 10^-2.
Therefore, the correct scientific notation for the percent yield is 6.55 * 10^-2 or 6.55%.
In summary, your calculations for the theoretical yield and percent yield are correct. Make sure to double-check your numbers and units to ensure accuracy. Good luck with your assignment!