ChemistryGrade 11Energy Changes and Electrochemistry

Electrochemistry Lab: Galvanic Cell Voltage and Current

Build a galvanic cell, choose electrodes, change ion concentrations and salt bridge conductivity, then measure open-circuit voltage and current.

SimulationsLab index
Textbook unitEnergy Changes and ElectrochemistryGrade 11 Chemistry Unit 4
Keywordselectrochemistry, galvanic cell, voltage, current, electrodeMapped to available textbook headings
Practice modeManipulate, measure, explainUse the controls, then read the live evidence

Chemistry · Grade 11

Build a galvanic cell and measure electron flow

Choose electrode metals, tune ion concentrations and salt bridge conductivity, then measure voltage, current, and power through a load.

StatusStable cell
1

Standard cell: build a Zn/Cu galvanic cell. Find E°cell and verify: E°cell = E°cathode − E°anode.

2

Concentration effect: change electrolyte concentration. Does voltage change? This is the Nernst equation.

3

Electrolysis: switch to electrolytic mode. What minimum voltage reverses the reaction? Compare with spontaneous E°cell.

Voltmeter0.79V
Zn
Zn2+oxidation
Cu
Cu2+reduction
salt bridge
Load8 ohm
Open voltage1.10 V
Internal resistance3.15 ohm
Reaction quotient1.00
Electrochemistry insight

Galvanic cell: E = 0.79 V (spontaneous, ΔG < 0). Oxidation at anode (Zn), reduction at cathode (Cu). ΔG = −nFE.

Terminal voltage0.79 V
Current0.099 A
Power0.078 W
E standard1.10 V
Electron flow45%

Lab task

Find two cell setups above 0.80 V, then reduce salt bridge conductivity and observe how current changes while open voltage stays similar.

Observation rule

Electrode chemistry and ion concentration set the cell voltage. Salt bridge quality and load resistance control how much current can flow.

Mission

What to prove in this lab

  1. Relate electrode choice and ion concentration to cell voltage.
  2. Explain how salt bridge conductivity and load resistance affect current.
  3. Use voltage, current, and power readings to compare galvanic cell setups.