Question

 

This experiment consisted of:
- Phosphoric Acid 2 mL
- Methyl Anthranilate 0.21 mL
- Sodium Nitrite 0.399 g
- Diethyl Ether 3 mL
- Urea ~0.14 g
- Sodium Bicarb 1 mL

As well as sodium sulfate, but that was "as needed".

At the end, I had 0.05 g of the final product.

How do I begin to calculate the percent yield?

Answer 1

In this reaction  Methyl Anthranilate is giving the product methyl salicylate

if 1 mole of methyl anthranilate is giving 1 mole of methyl salicylate then yield is 100 %

for methyl anthranilate the the density is 1.168 g/cm³  

You have taken 0.21 ml

so by converting it in grams Density = weight/volume

Weight = density * volume

= 1.168 * 0.21

= 0.2452 g

molecular weight of  Methyl Anthranilate is 151.165 g

so no of moles you have taken = weight /molecular weight

= 0.2452 / 151.165

= 0.0016 moles ( 1 eq)

  

Again molecular weight of methyl salicylate is 152.149 g

So for 100% yield it should give weight = molecular weight * no.of moles = 152.149 * 0.0016

= 0.2434 g ( Theoritical value )

But you got product 0.05 g

By formula Yield = experimental value / Theoritical value * 100

= 0.05 / 0.2434 * 100

= 0.2054 * 100

= 20.54 %