Chemical Reaction Lab Report

Introduction, aim and hypothesis
Chemical reactions are accompanied by the release or absorption of energy. Reactions which release energy are described as exothermic and those which absorb energy are endothermic. The energy released in chemical reactions was previously stored as chemical potential energy in the reactants; this stored energy is called enthalpy.
The aim of this practical is to observe and classify chemical processes as endothermic or exothermic, based on the changes in temperature measured and the observations made.
If a chemical reaction produces products with more chemical potential energy than the reactants, then the reaction is endothermic; if the chemical potential energy present after the reaction occurs is lower than the chemical potential energy
(°C)
Final Temp. (°C)
Endothermic/ Exothermic
Sodium Hydroxide NaOH
16.5
19.8
Exothermic
Ammonium Chloride NH4Cl

15.5
Endothermic
Sodium Acetate NaCH3COO

16.2
Slightly endothermic
Sodium Chloride NaCl

16.5
Neither

Part B Ammonium Chloride and Barium Hydroxide
Equipment and procedures (In book)
Results (observations)
A white solid forms in the bottom of the test tube after vigorous shaking; the lowest temperature recorded was 9°C.
Part C Iron and Copper(II) Sulfate
Equipment and procedures (In book)
Results (observations)
The blue solution becomes clear and the steel wool gradually turns red. The wool also heats up to a maximum of 35°C.
Processing the data
Equations
NaOH(s) + H2O(l) → Na+(aq) + OH-(aq) + H2O(l) + ENERGY
NaOH(s) → Na+(aq) + OH-(aq) + ENERGY
NH4Cl(s) + H2O(l) + ENERGY → NH4+(aq) + OH-(aq) + H+(aq) + Cl- (aq)
NH4Cl(s) + H2O(l) + ENERGY → NH4OH(aq) + H+(aq) + Cl- (aq)
NaCH3COO(s) + H2O(l) ENERGY (Small amount) → Na+(aq) + CH3COO-(aq) H2O(l)
NaCH3COO(s) → Na+(aq) + CH3COO-(aq)
No reaction for NaCl and water so no equation
2NaCl(s) + Ba(OH)2(s) → BaCl2(aq) + 2NaOH(aq)
2Fe(s) + CuSO4(aq) → Cu2+(s) + Fe2SO4(aq)
Conclusion (Research all references in