Solid lithium hydroxide (lioh) is used in space vehicles to remove exhaled carbon dioxide (co2). the lithium hydroxide reacts with carbon dioxide to form solid lithium carbonate (li co; ) and liquid water. the balanced chemical equation is given by 2 lioh(s) + co2(g)→ li2co3(s) + h2o(l)
a. if only 1.00 mole of lioh is available to react with co2, how many moles of liquid water are produced? assume that co2 is not limiting.
b. if 3.00 moles of li cos are produced, how many grams of lioh were consumed?
c. how many grams of co2 can be absorbed by 12.50 g of lioh?

a) 0.5 mol H₂O b) 143.64 g LiOH c) 11.49 g CO₂

Explanation:

Considering the general chemical reaction, we also have the molecular mass for each component:

M LiOH = 23.94 g/mol

M CO₂ = 44 g/mol

M Li₂CO₃ = 73.88 g/mol

M H₂O = 18 g/mol

Then we should consider the stechiometry of the above chemical reaction in order to answer each item:

a) If we have 1 mol of LiOH, then:

2 moles LiOH = 1 mol H₂O

1 mol LiOH = 0.5 mol H₂O are produced

b) If we obtain 3 moles of Li₂CO₃, then:

1 mol Li₂CO₃ = 2 moles LiOH

3 moles Li₂CO₃ = 6 moles LiOH, and considering the molecular mass:

6x23.94 = 143. 64 g LiOH were consumed

c) If we have 12.50 g of LiOH, then:

47.88 g LiOH absorbes 44 g CO₂

12.50 g LiOH will abosrb 11.49 g CO₂

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.