Question

Xg 10. Bromine (63 g) and fluorine (60 g) are mixed to give bromine trifluoride. a) Write a balanced chemical reaction. b) What is the limiting reactant? c) Determine how many grams of the product will form if the percent yield of the reaction is 80%. d) Determine how many grams of the excess reactant is left unreacted.

please include the physical state of each element

Answer 1

Solution Bry+ F Br Fz (a) Balanced chemical equation is- Br + 3 F 2Br z Also, determining physical states Bra (aq) + 3 F (g) 2 Br Fz (4) (b) Moles of Brg 2) 63g =) 07875 80 g-mol Moles of ) 3 157 F₂ =) 60g 19g med Molar ratio of Br = 0.7875 = 0.7875 Molar ratio of F22) 3.157 = 1.052 Molar ratio of Bry < Molar ratio of Fa Hence, Br is limiting reagent

co Date II I mole of Bry & 2 moles of By F 0.7875 moles of Br = 2 0 7875 = 1.575 moles of BrĄ Theoritical Yeild (in grams) 1.575x 137 g. med ) 215.775 g 7. Yeilda Yeild LLLLLLLLLLL 222 Actual Yeild Theoritical Actual Yeild 215.789 0.8 = Actual Heild >> 172-624 Answers (172.6 g (d) Imole of Bry i 3 moles of FL 0.7875 moles of Bra E 3 0.7875 - 2.3625 moles No of moles left: 3.157 -2.3625 - 0.79 45 moles Henar Amount in amount Grand 2) 0.79 45 x 19 g mol- [15.09 gif