Final answer:
To determine the moles of LiOH needed to react with 25.5 g of CO₂, divide the mass of CO₂ by its molar mass to get the moles of CO₂, then use the stoichiometry of the reaction between LiOH and CO₂ to find the moles of LiOH needed. The calculation leads to 1.16 moles of LiOH.
Step-by-step explanation:
To determine how many moles of LiOH are needed to react completely with 25.5 g of CO₂, one should use stoichiometry, which involves mole-to-mole conversions based on a balanced chemical reaction equation. The balanced reaction between lithium hydroxide (LiOH) and carbon dioxide (CO₂) is:
- 2 LiOH + CO₂ → Li₂CO₃ + H₂O
According to this equation, 2 moles of LiOH react with 1 mole of CO₂. The molar mass of CO₂ given is 44.01 g/mol. To find the number of moles of CO₂ present in 25.5 g, divide 25.5 g by the molar mass:
Number of moles of CO₂ = 25.5 g / 44.01 g/mol
Carrying out this calculation gives approximately 0.579 moles of CO₂. Since the stoichiometry of the reaction shows that 2 moles of LiOH are required for every mole of CO₂, we multiply the moles of CO₂ by 2:
Moles of LiOH needed = 0.579 moles of CO₂ × 2
This equals 1.158 moles of LiOH. Therefore, the correct answer is:
(c) 1.16 moles of LiOH are needed to react completely with 25.5 g of CO₂.