更新1:
chemistry gas laws?
2020-09-23 5:29 am
Solid lithium hydroxide is used to "scrub" CO2 from the air in spacecraft and submarines; it reacts with the CO2 to produce lithium carbonate and water. What volume in liters of CO2 at 23°C and 752 torr can be removed by reaction with 440 g of lithium hydroxide?
回答 (2)
2020-09-23 6:17 am
✔ 最佳答案
Molar mass of LiOH (lithium carbonate) = (6.9 + 16.0 + 1.0) g/mol = 23.9 g/molBalanced equation for the reaction:
2LiOH + CO₂ → Li₂CO₃ + H₂O
Mole ratio LiOH : CO₂ = 2 : 1
Moles of LiOH reacted = (440 g) / (23.9 g/mol) = 18.41 mol
Moles of CO₂ removed = (18.41 mol) × (1/2) = 9.205 mol
Consider the CO₂ absorbed:
Pressure, P = 752/760 atm
Volume, V = ?
Temperature, T = (273 + 23) K = 296 K
No. of moles, n = 9.205 mol
Gas constant, R = 0.08206 L atm / (mol K)
Gas law: PV = nRT
Then, V = nRT/P
Volume of CO₂ removed, V = 9.205 × 0.08206 × 296 / (752/760) L = 226 L
2020-09-23 5:42 am
Find moles. Divide 440 g by the molecular weight of LiOH (about 24 g/mole).
The reaction is: 2LiOH + CO2 --> 2LiCO3 + H2O
So divide the moles of LiOH by two to find the number of moles of CO2 consumed.
Now use the gas law equation (PV = nRT) to find V remembering to put the temperature into degrees K.
The reaction is: 2LiOH + CO2 --> 2LiCO3 + H2O
So divide the moles of LiOH by two to find the number of moles of CO2 consumed.
Now use the gas law equation (PV = nRT) to find V remembering to put the temperature into degrees K.
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