2. At room temperature, consider a cell consisted of a Cl2 (0.010 atm)|CI (1 M) half-cell connected to a Cl2 (0.50 atm)|Cl¯ (1 M) half-cell. Assume rigid half-cells so that the volumes of respective cells remain constant, and Cl2 to be ideal gas. (a) Determine which half-cell will be the anode using Thermodynamics. (b) Calculate half reaction potentials using the Nernst equation, and calculate the cell potential. For the Cl2 (0.50 atm)|Cl (1 M) half-cell, Cl2 (0.50 atm) + e → Cl (1 M):
Science behind corrosion-test
Corrosion is defined as an activity that transforms refined metals into more chemically stable forms such as oxide, hydroxide, carbonate, or sulfide. It refers to the slow decomposition of things (typically metals); thanks to chemical and/or electrochemical reactions with their surroundings. Corrosion engineering is the science of preventing and controlling corrosion.
Corrosion
Corrosion is defined as an activity that transforms refined metals into more chemically stable forms such as oxide, hydroxide, carbonate, or sulfide. It refers to the slow decomposition of things (typically metals); thanks to chemical and/or electrochemical reactions with their surroundings. Corrosion engineering is the science of preventing and controlling corrosion.
For a)I know that Cl2 (.010 atm)|Cl- is the anode but not sure how to figure that out?
For b) I know the answer is 1.35V but would like to see how that is calculated
Step by step
Solved in 3 steps with 3 images
