Question Detail
Question
How many moles of KBr are required to prepare 0.0700 moles of Br₂ according to the reaction KBrO₃ + 6HNO₃ = 6KNO₃ + 3Br₂ + 3H₂O?
Correct Answer
Option A is the correct answer.
Detailed Explanation
The equation as written has KBrO₃, not KBr. It appears there is a typo; the reaction likely involves KBr. From 6KNO₃ on the right, the K⁺ comes from KBr? The correct balanced equation for Br₂ production from KBr and KBrO₃ in acid is: 5KBr + KBrO₃ + 6HNO₃ → 3Br₂ + 6KNO₃ + 3H₂O. For 3 mol Br₂, need 5 mol KBr. For 0.0700 mol Br₂, KBr = (5/3)×0.0700 = 0.1167 mol ≈ 0.1166 mol.
Hint
Balance the redox reaction correctly to find the stoichiometric ratio.