You're asking about the reaction of bromine trifluoride (BrF₃), not "0.196 trifluoride." Here's how we can approach this problem:

Understanding the Reaction

Bromine trifluoride (BrF₃) is a powerful oxidizing agent and can react with many substances, including itself. One common reaction is the disproportionation reaction where BrF₃ reacts to form bromine (Br₂) and bromine pentafluoride (BrF₅):

3 BrF₃ → Br₂ + 2 BrF₅

Stoichiometry and Calculation

* Balancing the Equation: The equation above is already balanced. This means that 3 moles of BrF₃ react to form 1 mole of Br₂.

* Moles of BrF₃: You're given 0.196 moles of BrF₃.

* Moles of Br₂: Using the stoichiometric ratio from the balanced equation:

(0.196 moles BrF₃) * (1 mole Br₂ / 3 moles BrF₃) = 0.0653 moles Br₂

Therefore, 0.0653 moles of bromine will be formed upon the complete reaction of 0.196 moles of bromine trifluoride.