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Problem: Chlorine dioxide gas (ClO2) is used as a commercial bleaching agent. It bleaches materials by oxidizing them. In the course of these reactions, the ClO2 is itself reduced.One method of preparing ClO2 is by the reaction of chlorine and sodium chlorite:Cl2(g) + 2 NaClO2(s) → 2 ClO2(g) + 2 NaCl(s)If you allow 15.5 g of NaClO2 to react with 2.00 L of chlorine gas at a pressure of 1.50 atm at 21 oC, how many grams of  ClO2 can be prepared?

🤓 Based on our data, we think this question is relevant for Professor Ratliff's class at USF.

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Problem Details

Chlorine dioxide gas (ClO2) is used as a commercial bleaching agent. It bleaches materials by oxidizing them. In the course of these reactions, the ClO2 is itself reduced.

One method of preparing ClO2 is by the reaction of chlorine and sodium chlorite:
Cl2(g) + 2 NaClO2(s) → 2 ClO2(g) + 2 NaCl(s)
If you allow 15.5 g of NaClO2 to react with 2.00 L of chlorine gas at a pressure of 1.50 atm at 21 oC, how many grams of  ClO2 can be prepared?

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