Respuesta :
Answer : The theoretical yield of water in this reaction is 360 g.
Solution : Given,
Mass of
Mass of
Mass of
Molar mass of = 44 g/mole
Molar mass of = 24 g/mole
Molar mass of = 18 g/mole
First we have to calculate the moles of and .
Moles of =
Moles of =
The given balanced chemical reaction is,
From the given reaction, we conclude that
1 mole of react with 2 mole of
20 moles of requires of
But the actual moles of = 42 moles
Excess moles of = 42 - 40 = 2 moles
So, is the limiting reagent.
Now we have to calculate the mass of .
From the reaction, we conclude that
1 mole of gives 1 mole of
20 moles of gives 20 moles of
Mass of = Moles of × Molar mass of
Mass of = 20 moles × 18 g/mole = 360 g
The experimental yield of = 325 g
Therefore, the theoretical yield of = 360 g
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Answer:
the theoretical yield is 360 g of H2O
Explanation:
mass of LiOH to mol of LiOH
1000 g of LiOH * (1 mol of LiOH/24 g of LiOH) = 41.67 mol of LiOH
mass of CO2 to mol of CO2
880 g of CO2 * (1 mol of CO2/44 g of CO2) = 20 mol of LiOH
mol divided by stoichiometric coefficient:
LiOH: 41.67 mol/2
CO2: 20 mol/1
Given that this ratio is smaller for CO2, then CO2 is the limiting reactant.
If 20 mol of CO2 reacts, then 20 mol of H2O are produced.
mol of H2O to mass of H2O:
20 mol of H2O * (18 g of H2O/1 mol of H2O) = 360 g of H2O
And that is the theoretical yield of the reaction.
Actual yield is 325 g of H2O, then the percent yield is:
percent yield = (actual yield/theoretical yield) x 100%
percent yield = (325/360) x 100% = 90.28%
