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. (a) What is the Lewis structure for ClO2? (b) Why do you think that ClO2 is reduced so readily? (c) When a ClO2 molecule gains an electron, the chlorite ion, ClO2 -, forms. Draw the Lewis structure for ClO2 -. (d) Predict the O—Cl—O bond angle in the ClO2 - ion. (e) 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 15.0 g of NaClO2 to react with 2.00 L of chlorine gas at a pressure of 1.50 atm at 21 °C, how many grams of ClO2 can be prepared?
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