Question
The carbondioxide generated by the personnel in the artificial atmosphere of submarines and space craft must be removed from the air and oxygen recovered. Submarine design teams have investigated the use of potassium super oxide (KO2) as an air purified because this compound reacts with CO2 and release oxygen
4KO2(s) + 2CO2(g) = 2K2C3(s) +3O2(g)
Calculate the mass of KO2 needed to react with 50 L of CO2 at 25 degrees Celsius and 1.0atm.
4KO2(s) + 2CO2(g) = 2K2C3(s) +3O2(g)
Calculate the mass of KO2 needed to react with 50 L of CO2 at 25 degrees Celsius and 1.0atm.
Answers
GPT 3.5
First, we need to calculate the number of moles of CO2 in 50 L at 25 degrees Celsius and 1.0 atm using the ideal gas law:
PV = nRT
(1.0 atm)(50 L) = n(0.0821 L.atm/mol.K)(298 K)
n = 2 moles
From the balanced chemical equation, we can see that the molar ratio of KO2 to CO2 is 4:2. Therefore, the molar ratio of KO2 to CO2 is 4:2 or 2:1.
Since we have 2 moles of CO2, we will need 2 moles of KO2 to react with it.
The molar mass of KO2 is 71.099 g/mol.
Therefore, the mass of KO2 needed is:
2 moles KO2 x 71.099 g/mol = 142.198 g
So, the mass of KO2 needed to react with 50 L of CO2 at 25 degrees Celsius and 1.0 atm is 142.198 grams.
PV = nRT
(1.0 atm)(50 L) = n(0.0821 L.atm/mol.K)(298 K)
n = 2 moles
From the balanced chemical equation, we can see that the molar ratio of KO2 to CO2 is 4:2. Therefore, the molar ratio of KO2 to CO2 is 4:2 or 2:1.
Since we have 2 moles of CO2, we will need 2 moles of KO2 to react with it.
The molar mass of KO2 is 71.099 g/mol.
Therefore, the mass of KO2 needed is:
2 moles KO2 x 71.099 g/mol = 142.198 g
So, the mass of KO2 needed to react with 50 L of CO2 at 25 degrees Celsius and 1.0 atm is 142.198 grams.