Final answer:
To find out how many grams of ClO₂ can be prepared, you calculate the moles of chlorine gas with the ideal gas law and then apply stoichiometry using the balanced chemical reaction between NaClO₂ and Cl₂.
Step-by-step explanation:
The chemical reaction between sodium chlorite (NaClO₂) and chlorine gas (Cl₂) is used to produce chlorine dioxide (ClO₂). To determine the amount of ClO₂ that can be prepared, we must first use the ideal gas law to calculate the number of moles of Cl₂ present, then use stoichiometry to find out how much ClO₂ can be produced from 15.0 g of NaClO₂.
Using the ideal gas law PV=nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature in Kelvin, we can find the moles of Cl₂. The pressure P is given as 1.50 atm, the volume V is 2.00 L, the ideal gas constant R is 0.0821 L·atm/K·mol, and the temperature T is (21+273) K.
After calculating the moles of Cl₂, we use the stoichiometry of the balanced chemical equation to find out how many moles of ClO₂ are produced per mole of NaClO₂, and thereby determine the mass of ClO₂ produced from 15.0 g of NaClO₂. Finally, convert the moles of ClO₂ to grams using its molar mass.