The balanced chemical formula is
1 IBr3 + 4 F2 → 1 IF5 + 3 BrF
Given 3.79×10-3 g of IBr3, determine the mass (in grams) of F2 that is required to completely react with all of the IBr3.
1 IBr3 + 4 F2 → 1 IF5 + 3 BrF
Given 3.79×10-3 g of IBr3, determine the mass (in grams) of F2 that is required to completely react with all of the IBr3.
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IBr3 + 4 F2 → IF5 + 3 BrF
(3.79 × 10^-3 g IBr3) / (366.6168 g IBr3/mol) × (4 mol F2 / 1 mol IBr3) ×
(37.9968 g F2/mol) = 0.00157 g F2
(3.79 × 10^-3 g IBr3) / (366.6168 g IBr3/mol) × (4 mol F2 / 1 mol IBr3) ×
(37.9968 g F2/mol) = 0.00157 g F2