Question

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?

Answer 1

916.74g of CO2

Step-by-step 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.