Show your work for all calculations. When 1.104 grams of iron metal are mixed wi
ID: 547725 • Letter: S
Question
Show your work for all calculations. When 1.104 grams of iron metal are mixed with 26.023 grams of hydrochloric acid in a coffee cup calorimeter, the temperature rises from 25.2 °C to a maximum of 33.5 °C. The reaction that occurs is given below. 1. 2 Fe (s) + 6 HCl (aq) 2 FeCl3 (aq) + 3 H2 (g) a) Determine the amount of heat (in J) absorbed by the reaction mixture. Assume that the specific heat capacity of the mixture is the same as the specific heat capacity of water. b) How much heat (in J) was released by the reaction that occurred? c) Is this reaction exothermic or endothermic? Is tection positive or negative? d) Under constant pressure conditions (as used in this experiment), the heat released by the reaction equals the reaction enthalpy, qreleasedAHreaction Determine AHreaction in Joules per gram of metal used (J/g). e) Determine AHreaction in kilojoules per mole of metal used (kJ/mol). f) Determine Hreaction in kilojoules for the balanced reaction equation provided (KJ).Explanation / Answer
Mass of the mixture = mass of iron + mass of hydrochloric acid = 1.104+26.023=27.127 gm
No heat is absorbed by the reaction mixture, the reaction releases heat.
Heat released by the reaction mixture= mass of mixture* specific heat* rise in temperature =-27.127*4.184*(33.5-25.2) =-942joules
Since heat is released during the course of reaction, the reaction is exothermic. deltaH is –ve.
Heat released /gm = 942/1.104 J/gm=853.3 J/gm
Moles of metal = mass of meta/ atomic weight of metal= 1.105/56 =0.0197
Heat released/ mole of methal= 942/0.0197 J/mole=47783 J/mole= 47.783 Kj/mole
1 mole of Fe released = 47.783 Kj
2 mole of Fe reacting as per the reaction are =2*47.783 Kj= 95. 6 Kj
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