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13 May 2018

so i have an experiment where i need to figure out the limiting reagent using 1.6 ml of a solution containing 58 mg acetone and ethanol. and 0.212 g of benzaldehyde. now i figured out the second part, but how do i calculate the acetone and ethanol mols? and which will be my limiting reagent?

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My teacher gives us tables to fill out, and I am really confused about how to go about it. Usually she gives us a few bits of information, but I need to learn how to do the conversions on my own. A table usually looks like this (with some procedure text):

compound	mp/bp, C	MW (g/mol)	equi	mmol	g	density (g/mL)	mL
thiamine-HCl	mp, 260 (dec)	337.3				(solid)	XXX
benzaldehyde	bp, 178-179					1.044
NaOH, 10% (w/v)	XXX	40.0				XXX

This table is an example for the formation of benzoin. The procedure involves .420 g thiamene HCl, 1.0 mL 10% NaOH, and 1.20 mL of benzaldehyde. I can fill in those things, but I don't know how to fill in the other blanks. For example, how do you calculate equiv (from any of the above)?

From here, how do I calculate theoretical yield? I know that I need to start with the limiting reagent, but how do I determine which one that is?

Thanks!!!! I can usually get help from my friends, but I need to know how to do these calculations (specifically equiv and mmol) on my own.

I did a chem lab where we made a coordination compound of Fe(III)KTOF3.

I need to figure out which is the limiting reagent, FeCl3, or KTOF3.

Here is the balanced equation: 3K2C204*H20+FeCl3. I know this means the equation has a 3:1 ratio.

I used 12.012 g of K2C204*H20, I know the molar mass is 184.231 g/mol. Which means I used 0.065201 moles of KTOF3 12.012g/ molar mass 184.231 is 0.065201 moles of KTOF3.

What is getting me stuck is the FeCl3. We used 7.9 ml of it, the concentration of it was 1.85 molar, and I know the molecular weight (126.751g).

How do I calculate the moles of FeCl3, so I can calculate the limiting reagent, theoretical yield, and the experimental yeild?

So I did a titration lab where were reacted various amounts of Mg with 10mL of HCL and then neutralized the raction with NaOH. I have my table of values for Mass of Mg (g), Initial Volume NaOH (mL), Final Volume NaOH (mL), End Point Volume (mL), Limiting Reagent (Mg or HCL). There is a Titration table I need to fill in that asks for Moles of Mg (mol), Moles of NaOH (mol) and Moles of H⁺ reacting with Mg (mol). I have the Moles of Mg calculated and I also have Moles of NaOH (mol) calculated but how do I go about finding Moles of H⁺ reacting with Mg. The manual says I can use: Moles of H⁺ total - moles of H⁺ excess = moles H⁺ reacting with metal. Where could I obtain those numbers.

I had in my notes to take Moles of Mg - Moles of NaOH and that gives the value but the problem with I am getting with that method is that if my limiting reagent is Mg then my Moles of H⁺ calculation ends up being a negative number.

My formula for calculating Moles of Mg is (Mass of Mg starting) * (1Mol/24.31g) = Moles of Mg

My formula for Calculating Moles of NaOh is: (End Point Volume)*(1L/1000mL)*(.3M HCL/1L) = Moles of NaOH

Thanks!

Some examples of my numbers would be

Moles of Mg = .001, Moles of NaOH = 8.58*10^-3 so that gives me a -7.6*10^-3 but I don't know if that is correct. Any help?

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so i have an experiment where i need to figure out the limiting reagent using 1.6 ml of a solution containing 58 mg acetone and ethanol. and 0.212 g of benzaldehyde. now i figured out the second part, but how do i calculate the acetone and ethanol mols? and which will be my limiting reagent?

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