Electrochemistry Lab Report
Introduction
A Voltaic Cell (also known as a Galvanic Cell) is an electrochemical cell that uses spontaneous redox reactions to generate electricity. It consists of two separate half-cells. A half-cell is composed of an electrode (a strip of metal, M) within a solution containing Mn+ ions in which M is any arbitrary metal. The two half cells are linked together by a wire running from one electrode to the other. A salt bridge also connects to the half cells.
Through electrochemistry, these reactions are reacting upon metal surfaces, or electrodes. An oxidation-reduction equilibrium is established between the metal and the substances in solution. When electrodes are immersed in a solution containing ions of the same metal, it is called a half-cell. Electrolytes are ions in solution, usually fluid, that conducts electricity through ionic conduction. Two possible interactions can occur between the metal atoms on the electrode and the ion solutions.
1. Metal ion Mn+ from the solution may collide with the electrode, gaining "n" electrons from it, and convert to metal atoms. This means that the ions are reduced.
2. Metal atom on the surface may lose "n" electrons to the electrode and enter the solution as the ion Mn+ meaning that the metal atoms are oxidized.
When an electrode is oxidized in a solution, it is called an anode and when an electrode is reduced in solution. it is called a cathode.1
Figure 1 A voltaic cell
Research Question: What is the effect of decreasing the activity of the metal pairs used with Cu to make a voltaic cell, on the voltage of the cell when room temperature, 18.0 ℃, room pressure, 1068 hPa, molarity and volume of electrolytes used, 1M – 50 mL, surface area of electrodes, 6cm x 3cm and type of salt bridge, KOH, is kept constant in each trial?
Aim: The aim of this investigation is to determine the effect of activity of metal pairs by changing the electrodes used on a half cell and keeping the other constant, Cu, under same
A Voltaic Cell (also known as a Galvanic Cell) is an electrochemical cell that uses spontaneous redox reactions to generate electricity. It consists of two separate half-cells. A half-cell is composed of an electrode (a strip of metal, M) within a solution containing Mn+ ions in which M is any arbitrary metal. The two half cells are linked together by a wire running from one electrode to the other. A salt bridge also connects to the half cells.
Through electrochemistry, these reactions are reacting upon metal surfaces, or electrodes. An oxidation-reduction equilibrium is established between the metal and the substances in solution. When electrodes are immersed in a solution containing ions of the same metal, it is called a half-cell. Electrolytes are ions in solution, usually fluid, that conducts electricity through ionic conduction. Two possible interactions can occur between the metal atoms on the electrode and the ion solutions.
1. Metal ion Mn+ from the solution may collide with the electrode, gaining "n" electrons from it, and convert to metal atoms. This means that the ions are reduced.
2. Metal atom on the surface may lose "n" electrons to the electrode and enter the solution as the ion Mn+ meaning that the metal atoms are oxidized.
When an electrode is oxidized in a solution, it is called an anode and when an electrode is reduced in solution. it is called a cathode.1
Figure 1 A voltaic cell
Research Question: What is the effect of decreasing the activity of the metal pairs used with Cu to make a voltaic cell, on the voltage of the cell when room temperature, 18.0 ℃, room pressure, 1068 hPa, molarity and volume of electrolytes used, 1M – 50 mL, surface area of electrodes, 6cm x 3cm and type of salt bridge, KOH, is kept constant in each trial?
Aim: The aim of this investigation is to determine the effect of activity of metal pairs by changing the electrodes used on a half cell and keeping the other constant, Cu, under same