Tag : electrochemistry

Electrochemistry Lab Experiment

Written by Elizabeth Data: Table 1: Measured Cell Potential Values Ecell (V) Cu/Zn 0.920 V Cu/Pb 0.646 V Zn/Pb 0.423 V   Table 2: Cell Potential Values for Reduction Half Reactions Ered (V) Cu2+ + 2e– –> Cu 0.34 V Zn2+ + 2e– –> Zn -0.58 V Pb2+ + 2e– –> Pb -0.31 V   Table 3: Elements of Cu/Pb Cell in Thermodynamic Study Temp (°C) Temp (K) ΔGrxn (kJ) Ecell (V) 76.0 °C 349 K -157.8 kJ 0.818 V 66.0 °C 339 K -158.8 kJ 0.823 V 56.0 […]

Comparing Tris-2,2’-bipyridine Complexes of Iron (II) and Ruthenium (II) through Spectroscopy and Electrochemistry

Written by Johanna ABSTRACT: This experiment effectively determined the differences between Iron (II) and Ruthenium (II) Tris-2,2’-bipyridine complexes through the comparison of absorption and emission spectroscopy and cyclic voltammetry.  In both the UV/Vis absorption and emission spectra, the Ru (II) complex shows far greater molar absorptivity values and fluorescence.  The iron complex does not fluoresce.  The MLCT peaks in the UV/Vis spectra correspond to the energy of the t2g à t2g*  or HOMO à LUMO transitions, 2.64 x 105 J/mol […]

Electrochemistry and the Nerst Equation

Objectives: 1. Measure the electrical potential of a zinc/iron battery cell at differing concentrations. 2. Construct an electrolytic cell. Procedure: Voltaic Cell 1. Prepare a 100mL of 0.1M Iron (II) Sulfate solution in a 150mL beaker and place the iron strip in the solution. 2. Prepare a 100mL of 0.1M Zinc Sulfate solution in a 150mL beaker and place the zinc strip in the solution. 3. Connect the beakers using the plastic bridge, which must be filled with a KCl […]