When chlorine gas (Cl2) reacts with oxygen gas (O2), they produce chlorine dioxide gas (ClO2). In this specific case, we have 0.70 liters of Cl2 reacting with 1.4 liters of O2. Based on the balanced reaction:
2 Cl2 (g) + 2 O2 (g) → 4 ClO2 (g),
we can observe that two volumes of chlorine react with two volumes of oxygen to produce four volumes of chlorine dioxide.
From our given conditions, 0.70 L of Cl2 would react with the amount of O2 following the stoichiometric ratio. Since 1.4 L of O2 is twice the volume needed for complete reaction of 0.70 L of Cl2, we will use the equation ratios to determine the reaction’s completion.
This indicates that chlorine gas is the limiting reagent since it is available in a smaller ratio compared to the amount of oxygen. After the reaction, we will have some unused oxygen remaining. Consequently, all of the Cl2 will be consumed, producing ClO2 gas from the complete reaction of 0.70 L of Cl2, which generates 1.4 L of ClO2 under the same temperature and pressure conditions.
In summary, when 0.70 L of Cl2 reacts with 1.4 L of O2, all of the chlorine gas is used up, and the products primarily consist of chlorine dioxide gas, while there will be excess oxygen remaining in the system.