# 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.

84% (472 ratings) ###### 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?