Question

The carbon dioxide generated by personnel in the artificial atmosphere of submarines and spacecraft must be removed from the air and the oxygen recovered. Submarine design teams have investigated the use of potassium superoxide (KO2) as an air purifier. This compound reacts with carbon dioxide to produce solid potassium carbonate and oxygen gas. Calculate the mass of KO2 needed to react with 5.0 × 101 L of carbon dioxide at 25 ºC and 1.00 atm.

Answer #1

**given that**

**K02 reacts with C02 to give K2C03 and 02**

**so**

**the balanced chemical equation is**

**2K02 + C02 ---> K2C03 + 1.5 02**

**now**

**for ideal gases such as C02**

**PV = nRT**

**so**

**using the given values**

**1 x 50 = n x 0.0821 x 298**

**n = 2.04367**

**so**

**moles of C02 = 2.04367**

**now**

**consider the reaction**

**2K02 + C02 ---> K2C03 + 1.5 02**

**we can see that**

**moles of KO2 needed = 2 x moles of CO2**

**so**

**moles of KO2 needed = 2 x 2.04367**

**moles of KO2 needed = 4.08734**

**now**

**we know that**

**mass = moles x molar mass**

**so**

**mass of KO2 needed = 4.08734 x 71**

**mass of KO2 needed = 290**

**so**

**290 grams of KO2 is needed**

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