Question

The overall reaction in commercial heat packs can be represented as the reaction below. 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s), ΔH = -1652 kJ (a) How much heat is released when 4.23 mol iron is reacted with excess O2? (b) How much heat is released when 1.48 mol Fe2O3 is produced? c) How much heat is released when 1.34 g iron is reacted with excess O2? (d) How much heat is released when 13.10 g Fe and 2.05 g O2 are reacted?

Answer 1

Tu Yeahon л – 4 fe (s) + 302 () -72,0,($) OH -1652 kJ. 1 4 mol amol amol So we have that 4 moles of for reacts with 3 moles of 82 to form a moles of Food and in this process a heat of 1652 kJ is released. (a) 4 mol of iron releases 1652 kJ heat. 4.3 mol of iron will produe = 1652 x 413 kJ = 1775.9 kJ of energy. (b) when 2 moles of Foz oz is produced, heat released = 1652 kJ 1652 a. when 1048 mol of Fe, O, is produced, heat - 1 271-68 2 = 1222.48 kJ. (C) Atomic mass of iron = 55.845 g/mol .. 4*55.845 = 22 3.38 g of iron produes heats 1652 kJ . : : Heat released by 1.348 Fe 12329641.34 kJ - 9.913 kJ. (d) If we convert into masses, 223.38 g of te reacts with 96 g of oxygen. So for complete reaction of 2005g of xygen iron required = 223.36 _x 2.05 g a 4.77g. So iron is present in excess and orggen is the limiting Heat released 16 LX 205 35.277 kJ, 96 96 reactant.