Dr. Bob222 Please don't get frustrated with me, I'm really trying to figure this out... UGH!!
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??
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
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???
Don't worry, I'm here to help you figure this out! Let's go through each part step by step:
a. To calculate the theoretical yield of Ti(s), you first need to determine the limiting reactant. This is the reactant that will be completely consumed and determines the maximum amount of product that can be formed. In this case, you need to compare the number of moles of TiCl4 and Mg.
To find the number of moles of TiCl4, you correctly used the equation:
moles of TiCl4 = (mass of TiCl4) / (molar mass of TiCl4)
Plugging in the given values:
moles of TiCl4 = 3.54×10^7 g / 189.68 g/mol = 186,508 moles (rounded to the nearest whole number)
To find the number of moles of Ti, you correctly used the equation:
moles of Ti = (mass of Ti) / (molar mass of Ti)
Plugging in the given values:
moles of Ti = 7.91×10^6 g / 47.88 g/mol = 165,275 moles (rounded to the nearest whole number)
Since the stoichiometric ratio between TiCl4 and Ti is 1:1, the limiting reactant here is TiCl4. This means that all the TiCl4 will be consumed during the reaction.
Now, to calculate the theoretical yield (TY) of Ti(s), you need to use the balanced equation. According to the equation, 1 mole of TiCl4 produces 1 mole of Ti. So, the theoretical yield of Ti(s) can be calculated as:
TY = moles of Ti = moles of TiCl4 = 186,508 moles.
b. The actual yield (AY) is given as 7.91×10^6 g. You correctly identified this value.
c. The percent yield is calculated using the formula:
% yield = (actual yield / theoretical yield) * 100
Plugging in the values:
% yield = (7.91×10^6 g / 186,508 moles) * 100 = 4.24%
Regarding the previous mention of a theoretical yield of 8.9E6, that might have been a typo or a miscalculation. The correct theoretical yield, as calculated above, is 186,508 moles.
I hope this clears up your confusion. If you have any further questions, feel free to ask!