A rebreathing mask contains potassium superoxide, KO 2 , which reacts with moist

Question

A rebreathing mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen:

4 KO2 (s) + 2 H2O (l) --> 4 KOH (s) + 3 O2 (g)

a) Calculate the amount of potassium superoxide required to supply a person's oxygen needs for one hour. Assume a person needs 418 J of energy for this period. Further assume that this energy can be equated to the heat of combustion of glucose, C6H12O6, to CO2 and H2O. From the amount glucose required to give 418 kJ, calculate the amount of oxygen consumed, and hence the amount of KO2 required.  H°f for glucose is -1273 kj/mol

b) The potassium hydroxide produced in the reaction in part a) reacts with carbon dioxide to give potassium carbonate and water. Write the balanced equation of the reaction between KOH and CO2.

c) What mass of KO2 is required to consume 37.0 g of CO2?

d) What mass of O2 is produced during this reaction?

Explanation / Answer

Balance

4KO2 (s) + 2H2O (l) -> 4KOH (s) + 3O2 (g)

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