Solid lithium hydroxide is used in space vehicles to remove exhaled carbon dioxide from the living environment by forming solid lithium carbonate and liquid water. 2 LiOH(s) + CO2(g) --> Li2CO3(s) + H2O(l)

If the space vehicle has 28.5. moles of LiOH and 21.7 moles of CO2. What mass of gaseous carbon dioxide can be absorbed by 1.00 kg of lithium hydroxide?

916.74g of CO2

Explanation:

We'll begin by calculating the number of mole in 1kg of LiOH. This can be achieved as shown below:

Molar mass of LiOH = 7 + 16 + 1 = 24g/mol

Mass of LiOH = 1kg = 1 x 1000 = 1000g

Mole of LiOH =...?

Mole = mass /molar mass

Mole of LiOH = 1000/24

Mole of LiOH = 41.67 moles

Next, we shall determine the number of mole of CO2 absorbed by 1kg (41.67 moles) of LiOH. This is illustrated below:

2LiOH(s) + CO2(g) —> Li2CO3(s) + H2O(l)

From the balanced equation above,

2 moles of LiOH reacted with 1 mole of CO2.

Therefore, 41.67 moles of LiOH will react with = (41.67x 1)/2 = 20.835 moles of CO2.

Finally, we shall convert 20.835 moles of CO2 to grams. This is illustrated below:

Molar mass of CO2 = 12 + (2x16 = 44g/mol

Mole of CO2 = 20.835 moles

Mass of CO2 =.?

Mole = mass /molar mass

20.835 = mass /44

Cross multiply

Mass of CO2 = 20.835 x 44

Mass of CO2 = 916.74g

Therefore, 916.74g of CO2 will absorbed.