this reaction makes potassium superoxide useful in a self-contained breathing apparatus. how much o2 could be produced from 2.41 g of ko2 and 4.62 g of co2?

Chemical reactions happen absolutely everywhere in our daily life. While we sometimes associate chemical reactions with only the sterile environment of test tubes and laboratories, nothing is farther from the truth. In fact, a wide range of transformations are creating a dizzying and almost incomprehensible series of new matter and energy changes in our world every second of every day.

Moles KO₂ = 2.41g/(71.1g/mole) = 0.034 moles

Moles CO₂ = 4.62g/(44g/mole) = 0.105 moles

4KO₂ + 2CO₂ → 2K₂CO₃ + 3O₂

The reaction requires twice as many moles of KO₂ than moles of CO₂. That means 0.105 mole of CO₂ would consume 0.034 moles of KO₂. But there is only have 0.034 moles of KO₂, so the limiting reagent is KO₂.

There are 3 moles of O₂ produced for every 2 moles of CO₂ consumed. In this case we'll assume all of the KO₂ reacts, so that should result in (3/4) × (0.034moles) = 0.025 moles of O₂ .

To get the mass, 0.025 mole × (32g/mole) = 0.823 grams O₂

Hence, 0.823 grams O₂ could be produced from 2.45 g of KO₂ and 4.62 grams o.f CO₂.

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