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?

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

The percent yield of potassium carbonate is, 85.33 %

Solution : Given,

Mass of = 150 g

Mass of = 90 g

Molar mass of = 212.27 g/mole

Molar mass of = 233.99 g/mole

Molar mass of = 138.205 g/mole

First we have to calculate the moles of and

The given balanced reaction is,

From the given reaction, we conclude that

2 moles of react with 1 mole of

0.7066 moles of react with moles of

But the moles of is, 0.3846 moles.

So, is an excess reagent and is a limiting reagent.

Now we have to calculate the moles of .

As, 2 moles of react to give 3 moles of

So, 0.7066 moles of react to give moles of

Now we have to calculate the mass of .

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 :

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

the formula would be mgso4

mgso[subscript]4

quartz

explanation: