Final answer:
The question refers to a chemical reaction to determine the volume of ClO₂ gas, but lacks the balanced equation required for calculations. Without it, we cannot calculate the molar ratio and subsequently the volume of ClO₂ produced from 15g of NaClO₂ at 1.2 atm and 45ºC.
Step-by-step explanation:
The question asks what volume of chlorine dioxide, ClO₂, can be produced at 1.2 atm and 45ºC when 15g of sodium chlorite, NaClO₂, reacts with an unstated stoichiometric amount of chlorine gas, Cl₂, under the same conditions.
To answer this, one would need the balanced chemical equation for the reaction between NaClO₂ and Cl₂ to determine the molar ratio of NaClO₂ to ClO₂.
Then, the moles of NaClO₂ are calculated using its molar mass and the given mass (15g). After calculating the moles of ClO₂ produced using the molar ratio from the balanced equation, the ideal gas law (PV=nRT) would apply to find the volume of ClO₂, with R as the ideal gas constant and T the temperature in kelvins.
However, as the balanced chemical equation necessary for calculating the stoichiometry of the reaction is not provided, it appears there may be a typo or omission in the question, which must be corrected to proceed further.