Chemistry, 29.06.2019 21:30 vannaht2003

Given the following reaction: 2k3po4 + al2(co3)3 = 3k2co3 + 2alpo4 if i perform this reaction with 150 g of potassium phosphate and 90 g of aluminum carbonate, what is my theoretical yeild in grams of potassium carbonate? if the reaction results in 125 g of potassium carbonate, what is my percent yeild?

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Answer from: kobeprewitt02

Answer : The theoretical yield of potassium carbonate is, 146.483 g

The percent yield of potassium carbonate is, 85.33 %

Solution : Given,

Mass of K_3PO_4 = 150 g

Mass of Al_2(CO_3)_3 = 90 g

Molar mass of K_3PO_4 = 212.27 g/mole

Molar mass of Al_2(CO_3)_3 = 233.99 g/mole

Molar mass of K_2CO_3 = 138.205 g/mole

First we have to calculate the moles of K_3PO_4 and Al_2(CO_3)_3

$\text{ Moles of }K_3PO_4=\frac{\text{ Mass of }K_3PO_4}{\text{ Molar mass of }K_3PO_4}=\frac{150g}{212.27g/mole}=0.7066moles$

$\text{ Moles of }Al_2(CO_3)_3=\frac{\text{ Mass of }Al_2(CO_3)_3}{\text{ Molar mass of }Al_2(CO_3)_3}=\frac{90g}{233.99g/mole}=0.3846moles$

The given balanced reaction is,

$2K_3PO_4+Al_2(CO_3)_3\rightarrow 3K_2CO_3+2AlPO_4$

From the given reaction, we conclude that

2 moles of K_3PO_4 react with 1 mole of Al_2(CO_3)_3

0.7066 moles of K_3PO_4 react with $\frac{1}{2}\times 0.7066=0.3533$ moles of Al_2(CO_3)_3

But the moles of Al_2(CO_3)_3 is, 0.3846 moles.

So, Al_2(CO_3)_3 is an excess reagent and K_3PO_4 is a limiting reagent.

Now we have to calculate the moles of K_2CO_3 .

As, 2 moles of K_3PO_4 react to give 3 moles of K_2CO_3

So, 0.7066 moles of K_3PO_4 react to give $\frac{3}{2}\times 0.7066=1.0599$ moles of K_2CO_3

Now we have to calculate the mass of K_2CO_3 .

$\text{ Mass of }K_2CO_3=\text{ Moles of }K_2CO_3\times \text{ Molar mass of }K_2CO_3$

$\text{ Mass of }K_2CO_3=(1.0599moles)\times (138.205g/mole)=146.483g$

The theoretical yield of potassium carbonate = 146.483 g

The experimental yield of potassium carbonate = 125 g

Now we have to calculate the % yield of potassium carbonate.

Formula for percent yield :

$\% yield=\frac{\text{ Theoretical yield}}{\text{ Experimental yield}}\times 100$

$\% \text{ yield of }K_2CO_3=\frac{125g}{146.483g}\times 100=85.33\%$

Therefore, the % yield of potassium carbonate is, 85.33%

Answer from: Quest

first, consult an activity series chart to determine if al is more reactive than fe. it is, so it will replace the fe. now, one can continue with the problem.

next, make sure you have a correctly balanced equation.

3feo + 2al ==> 3fe + al2o3

now, determine which reactant (feo or al) is in limiting supply.

moles feo present = 125 g x 1 mole/71.8 g = 1.74 moles

moles al present = 25.0 g x 1 mole/26.98 g = 0.927 moles

since from the balanced equation, it take 3 mol feo for every 2 mol al, al will be limiting.

you can determine this simply by dividing moles of each by their coefficient in the balanced equation. for example: 1.74/3 = 0.58 and 0.927/2 = 0.464. al is less, so it is limiting.

finally, using the stoichiometry in the balanced eq. determine mass of fe that can be produced from 0.927 moles of al.

0.927 moles al x 3 moles fe/2 moles al x 55.8 g/mole = 77.6 g

Answer from: Quest

a is the answer

explanation:

which statement about trans-fatty acids is false?

a. the conversion of cis-fatty acids to trans-fatty acids is inhibited by the presence of antioxidants.

hope this

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Given the following reaction: 2k3po4 + al2(co3)3 = 3k2co3 + 2alpo4 if i perform this reaction with...

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