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

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%