CO2(g) + 2 LiOH(s) → Li CO3(aq) + H2O In a one-person spacecraft, an astronaut exhales 880 g of CO2(g) (molar mass) per day. To prevent the buildup of CO2(g) in the spacecraft, a device containing LiOH(g) is used to remove the CO(g), as represented by the equation above. What mass of LiOH(s) (molar mass) is needed to react with all of the CO2(g) produced by an astronaut in one day?

958 g is the mass of LiOH that can react with all the CO₂

Explanation:

CO₂(g) + 2 LiOH(s) → Li₂CO₃(aq) + H₂O

We think in the reaction:

1 mol of carbon dioxide can react with 2 moles of lithium hydroxide.

First of all, we convert the mass of our reactant to mol:

880 g . 1mol /44g = 20 moles

As ratio is 1:2, 20 moles of CO₂ will react with 40 moles of LiOH.

Let's determine the mass:

40 mol .  23.95 g /1mol = 958 g