Electrochemistry

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  1. 4. A list of elements arranged in order of their standard electrode potentials.
  2. 8. The branch of chemistry that deals with the relationship between electrical energy and chemical reactions.
  3. 13. The extra voltage required in an electrolytic cell to drive a non-spontaneous reaction beyond its theoretical value.
  4. 15. An electrochemical cell that uses electrical energy to drive non-spontaneous chemical reactions.
  5. 17. Conductance (Conductivity) The ability of an electrolyte solution to conduct electricity, measured in siemens per meter (S/m).
  6. 21. A mathematical equation that relates the electrode potential to the concentrations of the reactants and products in a cell.
  7. 22. The amount of electric charge carried by one mole of electrons, approximately equal to 96,485 coulombs.
  8. 23. A reaction in which oxidation and reduction occur simultaneously, involving the transfer of electrons.
  9. 24. A substance that dissociates into ions in solution, allowing the solution to conduct electricity.
  10. 25. The electrode where oxidation (loss of electrons) occurs in an electrochemical cell.
  11. 26. The ability of an electrode to gain or lose electrons, measured in volts.
  12. 28. The deterioration of a metal as a result of chemical reactions with its environment, often involving electrochemical processes.
  13. 29. A law that states the limiting molar conductivity of an electrolyte is the sum of the contributions of its individual ions.
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  1. 1. The process of using electrical energy to drive a non-spontaneous chemical reaction.
  2. 2. Cell A rechargeable electrochemical cell, such as a lead-acid battery, which can be recharged and used multiple times.
  3. 3. A type of electrochemical cell that generates electrical energy from spontaneous redox reactions.
  4. 5. The electrode where reduction (gain of electrons) occurs in an electrochemical cell.
  5. 6. The electrode potential of a half-cell under standard conditions (1 M concentration, 298 K temperature, and 1 atm pressure).
  6. 7. The conductance of an electrolyte solution divided by its concentration, used to compare the conductive abilities of different electrolytes.
  7. 9. A device that generates electrical energy from chemical reactions or uses electrical energy to cause chemical changes.
  8. 10. The gain of electrons by a species in a chemical reaction.
  9. 11. The loss of electrons by a species in a chemical reaction.
  10. 12. A device used in galvanic cells to maintain electrical neutrality by allowing the flow of ions between two half-cells.
  11. 14. A conductor through which electric current enters or leaves an electrochemical cell.
  12. 16. A non-rechargeable electrochemical cell that provides energy until its reactants are used up (e.g., a dry cell or alkaline battery).
  13. 18. A process in which a metal is deposited onto a surface by passing an electric current through an electrolytic solution.
  14. 19. of Electrolysis Laws that quantify the relationship between the amount of substance produced or consumed at an electrode and the quantity of electric charge passed through the cell.
  15. 20. (SHE) A reference electrode with a defined potential of 0 volts, used as a standard for measuring electrode potentials in electrochemical cells.
  16. 22. An electrochemical cell that generates electricity through the continuous reaction of a fuel (such as hydrogen) with an oxidant (such as oxygen).
  17. 27. (EMF) The voltage difference between two electrodes in an electrochemical cell.