Question

In the following reaction at STP, how many liters of carbon dioxide will 1.8 moles of

lithium hydroxide (LiOH) absorb?
CO2(g) +2LIOH(s)-Li₂CO3(s)+H₂O(1)

Answer 1

Approximately 20.17 liters of carbon dioxide will be absorbed by 1.8 moles of lithium hydroxide (LiOH) at STP, utilizing the fact that 1 mole of a gas occupies 22.414 L at these conditions.

Step-by-step explanation:

In the reaction where carbon dioxide is absorbed by lithium hydroxide (LiOH), the stoichiometry of the reaction is such that 1 mole of CO2 is absorbed by 2 moles of LiOH. Given that 1.8 moles of LiOH is available, it can absorb 0.9 moles of CO2 (since 2 moles of LiOH are required for 1 mole of CO2, 1.8 moles will absorb half the amount of CO2).

At STP (Standard Temperature and Pressure), one mole of a gas occupies 22.414 liters. Therefore, 0.9 moles of CO2 would occupy:

0.9 moles × 22.414 L/mole = 20.1726 L

Approximately 20.17 liters of carbon dioxide will be absorbed by 1.8 moles of LiOH at STP.