(extra points+brainliest answer, : ) happy holidays) co2 + 2lioh = li2co3 + h2o to ensure that the air in the shuttle remains free of excess co2, engineers test the air-purification system. they combine 1.000 × 10^3 g lioh with 8.80 × 10^2 g co2. the reaction produces 3.25 × 10^2 g h2o. what is the theoretical yield of this test reaction? record answer to the nearest whole number. _g h2o

The theoretical yield of H₂O is 360 g.  

We have the masses of two reactants, so this is a limiting reactant problem.

We know that we will need a balanced equation with masses, moles, and molar masses of the compounds involved.  

Step 1. Gather all the information in one place with molar masses above the formulas and everything else below them.  

M_r:          44.01          23.95                  18.02

                 CO₂ +       2LiOH → Li₂CO₃ + H₂O

Mass/g: 8.80 × 10²  1.000 × 10³

Step 2. Calculate the moles of each reactant  

Moles of CO₂  = 8.80 × 10² g CO₂ × (1 mol CO₂ /44.01 g CO₂) = 20.00 mol CO₂

Moles of LiOH = 1.000 × 10³ g LiOH × (1 mol LiOH /23.95 g LiOH)

= 41.75 mol LiOH

Step 3. Identify the limiting reactant

Calculate the moles of H₂O we can obtain from each reactant.  

From CO₂ : Moles of H₂O = 20.00 mol CO₂ × (1 mol H₂O /1 mol CO₂)

= 20.00 mol H₂O

From LiOH: Moles of H₂O = 41.75 mol LiOH × (1 mol H₂O /2 mol LiOH)

= 20.88 mol H₂O

CO₂ is the limiting reactant because it gives the smaller amount of H₂O.

Step 4. Calculate the theoretical yield of H₂O.

Mass = 20.00 mol H₂O × (18.02 g H₂O /1 mol H₂O) = 360 g H₂O

The theoretical yield is 360 g H₂O.

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