How Much CO2 Can 1.90kg of KO2 Absorb?

[lorka150]

4KO2 + 2H2O --> 4KOH + 3O2
2KOH + CO2 --> K2CO3 + H2O

What mass of CO2 in kg can be absorbed by 1.90kg of KO2?

Molar masses are KO2 = 71.10g, CO2 = 44.01g
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So, would this make sense?
1.90kg KO2 x 1/71.10 x 4/4 x 56.11 = 1.499kg
then take that...
1.499g x 1/56.11 x 1/2 x 44.01 = 0.588kg (as the answer)



the 56.11 I had to figure out- they gave me the other molar masses...?

Thank you!

 

[Borek]

Why do you use water in reaction equations?

4KO₂ + 2CO₂ -> 2K₂CO₃ + 3O₂

But it doesn't change final result, as molar ratio of 4KO₂ and 2CO₂ is identical. 0.588 is OK.

 

[Blueshift5]

Yes, your calculations are correct. To determine the mass of CO2 that can be absorbed by 1.90kg of KO2, we first need to convert the mass of KO2 to moles by dividing by its molar mass (71.10g). Then, we use the mole ratio from the balanced equation (4 moles of KO2 : 1 mole of CO2) to find the moles of CO2 that can be absorbed. Finally, we convert the moles of CO2 back to mass by multiplying by its molar mass (44.01g) and converting to kg. The 56.11 is the molar mass of the compound K2CO3, which is needed in the second step of the reaction. Overall, your calculations and approach are correct in determining the mass of CO2 that can be absorbed by 1.90kg of KO2.