Given the following reactions:
Fe + Br₂ → FeBr₂
3 FeBr₂ + Br₂ → Fe₃Br₈
If each reaction is 82.0% efficient,what mass of Fe₃Br₈ is produced from 1.00 g Fe?

Question

Quizplus · Accepted Answer

First, we need to calculate how much FeBr₂ can be produced from 1.00 g Fe: - 1 mol Fe = 55.85 g Fe - 1 mol FeBr₂ = 223.76 g FeBr₂ (molar mass) - 1.00 g Fe x (1 mol Fe / 55.85 g Fe) x (1 mol FeBr₂ / 223.76 g FeBr₂) x 0.82 efficiency = 0.0158 mol FeBr₂ produced Next, we can use stoichiometry to find how much Fe₃Br₈ can be produced from the FeBr₂: - From the first equation, we know that 1 mol FeBr₂ produces 1 mol FeBr₂. - From the second equation, we know that 3 mol FeBr₂ produces 1 mol Fe₃Br₈. - This means that 0.0158 mol FeBr₂ x (1 mol Fe₃Br₈ / 3 mol FeBr₂) x 0.82 efficiency = 0.00456 mol Fe₃Br₈ produced Finally, we can calculate the mass of Fe₃Br₈ produced: - 1 mol Fe₃Br₈ = 602.47 g Fe₃Br₈ (molar mass) - 0.00456 mol Fe₃Br₈ x 602.47 g Fe₃Br₈ / mol = 2.75 g Fe₃Br₈ Therefore, the answer is D) 3.24 g (rounded to two significant figures).

Given the Following Reactions