Question

calculate the theoretical yield and the number of grams of hydrobenzoin that would form if every mole of the limiting reagent were converted 100% to product. Show all working and state the limiting reagent.

Answer #1

Here we know from each limiting reactant we get only one moles of hydrbenzoin. Mole ration between limiting reactant and the product so we get one mole of hydrobenzoin from one mole of reactant.

Now we use following molar mass of hydrobenzoin.

Molar mass of hydrobenzoin = 214.26 g /mol

Mass in g = Moles x molar mass

Mass in g = 1mol x 214.26 g = 214.26 g

Since we know when moles of limiting reactant used to find mole so product and further mass, we call mass is a theoretical mass.

**So the theoretical mass or yield = 214.26 g**

What is the theoretical yield in grams of the product from the
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(MW=178 g/mol) and 0.224 g of maleic anyhyride (MW= 98.1
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Which is the limiting reagent?
*Will someone please break down stoichiometry for me..
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1. You will be using 1.4 grams of salicylic acid to make
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Assuming that benzophenone (182.217 g/mol) is the limiting
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acid was added to 30 mL of diethyl ether and then transferred in a
seprartory funnel. 15 mL of 5% NaOH was added and the layers were
separated. This was done twice to separate the organic from the
aqueous layer then vaccum filtration was used to get the salt. I
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Limiting reagent and theoretical yield, product:
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Reaction : 1.5 grams m-nitrobenzoic acid, 12 mL methanol, .6 mL
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I started the calcualtions but I wasnt sure where to go
next:
.0006 L H2SO4 × 18.4 mol/L concentration H2SO4 = .01104 mol
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(a)calculate the theoretical yield of carbon dioxide
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(b) How many grams of excess reagent would be left
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Calculate the theoretical yield (in grams) of the precipitate
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B
C
Mass of empty test tube (g)
12.358g
7.675g
Drops of NiCl2
30
24
Drops of AgNO3
20
32
Conductivity of solution (μS/cm)
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Mass of precipitate and test tube (g)
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Tube C:
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.60 M Ag NO3

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