Problem: Potassium superoxide, KO2, is often used in oxygen masks (such as those used by firefighters) because KO2 reacts with CO2 to release molecular oxygen. Experiments indicate that 2 mol of KO2 (s) react with each mole of CO2(g).a. What mass of KO2(s) is needed to consume 18 g CO2(g)? b. What mass of O2(g) is produced during this reaction?

FREE Expert Solution

We’re being asked to calculate the mass of KO2 needed to consume 18 g of CO2 and the mass of oxygen (O2) produced by the reaction of 2 mol KO2.


For this problem, we need to do the following steps:

Step 1: Write and balance a chemical equation for the given reaction.

Step 2: Calculate the mass of KO2 needed to consume CO2.

Step 3: Calculate the mass of O2 produced.



Step 1: From the problem, the given reaction is:

KO2 + CO2 → K2CO+ O2


This equation is not yet balanced. To balance it, we have to make sure that the number of elements on both sides is equal.


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Problem Details

Potassium superoxide, KO2, is often used in oxygen masks (such as those used by firefighters) because KO2 reacts with CO2 to release molecular oxygen. Experiments indicate that 2 mol of KO2 (s) react with each mole of CO2(g).

a. What mass of KO2(s) is needed to consume 18 g CO2(g)? 

b. What mass of O2(g) is produced during this reaction?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Stoichiometry concept. You can view video lessons to learn Stoichiometry. Or if you need more Stoichiometry practice, you can also practice Stoichiometry practice problems.

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Based on our data, we think this problem is relevant for Professor Hoeger's class at UCSD.