Final answer:
To determine the mass of water required to react with Nitrogen dioxide and the volume of Nitrogen monoxide produced from water, we need to use stoichiometry and the ideal gas law.
Step-by-step explanation:
a. To determine the mass of water required to react with 15.5 L of Nitrogen dioxide (NO₂), we need to use the balanced equation and stoichiometry. According to the equation 3NO₂(g)+ H₂O₍ₗ₎ → HNO₃(aq) + NO(g), the molar ratio of NO₂ to H₂O is 3:1. First, convert the volume of NO₂ from liters to moles using the ideal gas law. Then, use the molar ratio to calculate the moles of H₂O needed. Finally, convert moles of H₂O to grams using the molar mass of water to find the mass of water required.
b. To find the volume of Nitrogen monoxide (NO) produced from 100.0 g of water, we can use the same process as in part a but in reverse. Start by calculating the moles of water using the molar mass. Then, use the molar ratio from the balanced equation to find the moles of NO produced. Finally, convert the moles of NO to the volume using the ideal gas law.