if 10.3 lithium sulfate react with an abundant amount of potassium phosphate, what mass of lithium phosphate can you expect to isolate?
lithium sulfate to lithium phosphate : 10.03 x 3 li3PO4 x 115.79 Lipo4 / 109.94 liSo4 / 3 LiSo4 = 10.9016179159
potassium phosphate to lithium phosphate: 56 x 3 li3po4 x 115.79 / 12.267 / 3 = 792.888236733
Im gussing potassium phosphate to lithium phosphate expect to isolate becuase its more?
I messed up the problem. potassium phosphate to lithium phosphate: 56 x 3 li3po4 x 115.79 / 212.267(forgot the 2) / 3 = 45.8213476424.
To determine the mass of lithium phosphate that can be isolated when 10.3 grams of lithium sulfate reacts with an abundant amount of potassium phosphate, you need to calculate the stoichiometry of the reaction.
Let's start by writing the balanced chemical equation for the reaction:
2 Li2SO4 + 3 K3PO4 -> 6 Li3PO4 + K2SO4
From the balanced equation, you can see that 2 moles of lithium sulfate (Li2SO4) react with 3 moles of potassium phosphate (K3PO4) to produce 6 moles of lithium phosphate (Li3PO4).
Next, you need to calculate the molar masses of the compounds involved:
- Molar mass of Li2SO4 = 109.94 g/mol
- Molar mass of K3PO4 = 212.27 g/mol
- Molar mass of Li3PO4 = 115.79 g/mol
Now, let's calculate the moles of lithium sulfate and potassium phosphate:
Moles of Li2SO4 = mass of Li2SO4 / molar mass of Li2SO4
= 10.3 g / 109.94 g/mol
= 0.0937 mol
Since the reaction is assumed to have an abundant amount of potassium phosphate, you can compare the moles of lithium sulfate and potassium phosphate to determine the limiting reagent. The reactant that produces fewer moles of the product (in this case, Li3PO4) will limit the amount of product formed.
Moles of K3PO4:Li3PO4 = 3:6
Using the moles of Li2SO4, you can calculate the moles of Li3PO4 formed:
Moles of Li3PO4 = 0.0937 mol x (6 mol Li3PO4 / 2 mol Li2SO4)
= 0.281 mol Li3PO4
Finally, calculate the mass of Li3PO4 using the moles and molar mass:
Mass of Li3PO4 = moles of Li3PO4 x molar mass of Li3PO4
= 0.281 mol x 115.79 g/mol
= 32.5 g
Therefore, you can expect to isolate approximately 32.5 grams of lithium phosphate. It seems that your calculation for the mass of lithium phosphate based on potassium phosphate is incorrect. The correct calculation shows that the mass of lithium phosphate formed from lithium sulfate is indeed greater than the mass formed from potassium phosphate.