First, we need to find the moles of CO2 in 50 L at 25°C and 1.0 atm:
PV = nRT
(1.0 atm)(50 L) = n(0.0821 L atm/mol K)(298 K)
n = 2 moles
According to the balanced chemical equation, 4 moles of KO2 react with 2 moles of CO2. Therefore, the moles of KO2 needed can be calculated as follows:
moles of KO2 = (4/2) * moles of CO2
moles of KO2 = 4 moles
The molar mass of KO2 is 71.10 g/mol. Therefore, the mass of KO2 needed to react with 50 L of CO2 is:
mass of KO2 = moles of KO2 * molar mass of KO2
mass of KO2 = 4 moles * 71.10 g/mol
mass of KO2 = 284.4 g
Finally, converting the mass to kilograms:
mass of KO2 = 0.2844 kg
Therefore, the mass of KO2 needed to react with 50 L of carbon dioxide is 0.2844 kg.
The carbon dioxide generated by the personnel in the artificial atmosphere of submarines and spacecraft must be removed from the air and the oxygen recovered. Submarine design teams have investigated the use of potassium superoxide (KO2) as an air purifier because this compound reacts with carbon dioxide and releases oxygen:
4KO2(s) + 2CO2(g) 2K2CO3(s) + 3O2(g).
Calculate the mass of KO2 needed to react with 50 L of carbon dioxide at 25oC and 1.0 atm.Convert your final answer to kilograms.
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