Question

What is the theoretical yield of this test reaction? Record answer to the nearest whole number.

Answer 1

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 2

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%