Calcium oxide can be used to "scrub" carbon dioxide from
air.
CaO (s) + CO2 (g) --> CaCO3 (s)
What mass of CO2 could be absorbed by 1.85 g of ?
Mass = g CO2
What volume would this CO2 occupy at STP?
Volume = L CO2
Calcium oxide can be used to "scrub" carbon dioxide from
air.
CaO (s) + CO2 (g) --> CaCO3 (s)
What mass of CO2 could be absorbed by 1.85 g of CaO(s)
Molar mass of CaO=56.08 g/mol
So moles of CaO = 1.85 g / 56.08 g/mol = 0.033 moles
Now one mole of CaO reacts with one mole of CO2
So 0.033 moles of CaO will react with 0.033 mole of CO2
Mass of CO2 = moles of CO2 Molar mass of CO2 = 0.033moles 44 g/mol = 1.5 g
What volume would this CO2 occupy at STP?
T = 273.15 K
P = 1 atm
n = 0.033 mole
R = 0.082L atm mol-1K-1
V = nRT/P = (0.033 mole 0.082L atm mol-1K-1 273.15 K) / 1 atm = 0.74 L
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