Electrode Potentials and Electrochemical Cells

• Who is the presenter of the video on AQA electrode potentials?

  Chris Harris
• What is the focus of the video presented by Chris Harris?

  AQA electrode potentials and electrochemical cells
• What type of chemistry does the video cater to?

  AQA A level chemistry
• How does this video differ from other resources?

  It specifically covers AQA specifications
• What additional resources are available on Chris Harris's YouTube channel?

  Revision videos and past paper walkthroughs
• What is the purpose of the slides available for purchase?

  To provide revision notes and study aids
• What is the main topic of the video?

  Electrode potentials and electrochemical cells
• What is a half cell in an electrochemical cell?

  One half of an electrochemical cell
• What materials can be used to construct a half cell?

  A metal dipped in its ions or platinum electrode
• What happens when a metal comes into contact with its ions in a half cell?

  A reaction occurs that is in equilibrium
• What is the equilibrium reaction involving Fe ions?

  Fe²⁺ + 2 electrons ⇌ Fe
• Why is platinum used as an electrode in some half cells?

  It is inert and has good conductivity
• What is an electrochemical cell made of?

  Two half-cells joined with a wire and salt bridge
• What does the voltmeter measure in an electrochemical cell?

  The potential difference between two half-cells
• From where do electrons flow in an electrochemical cell?

  From a more reactive metal to a less reactive one
• What happens to the zinc electrode during the reaction?

  It gets thinner as zinc converts to ions
• What occurs at the copper electrode during the reaction?

  Copper ions accept electrons and form copper metal
• What is the role of the salt bridge in an electrochemical cell?

  To complete the circuit and balance charges
• What is the standard hydrogen electrode used for?

  To measure standard electrode potential
• What are the standard conditions for the standard hydrogen electrode?

  298 K and 100 kPa
• What is the significance of the E_naught value?

  It indicates how easily a half cell gives up electrons
• How are electrode potentials typically presented?

  In reduced form with electrons included
• What does the acronym "no problem" help remember?

  The most negative half cell undergoes oxidation
• What does the term "redox reaction" refer to?

  A reaction involving reduction and oxidation
• What happens to the zinc half cell during the reaction?

  Zinc loses electrons and forms zinc ions
• What is the outcome of combining the half equations for zinc and copper?

  Zinc solid plus copper ions forms zinc ions and copper solid
• Why can't electrode potentials be measured alone?

  They require a reference like the standard hydrogen electrode
• What is the purpose of having a reference electrode?

  To allow global comparison of electrode potentials
• What is the setup for measuring the electrode potential of a copper half cell?

  Hydrogen gas at 298 K and 100 kPa with copper ions
• What type of half cell is used to measure electrode potential?

  Copper half cell
• What is the role of the platinum electrode in the setup?

  It serves as the inert conductor for the reaction
• What are the standard conditions for measuring electrode potential?

  298 Kelvin and 100 kPa
• Why is the concentration of H+ ions important in the setup?

  It must be 1 mole per dm³ for accuracy
• What concentration of copper ions is required in the beaker?

  1 mole per dm³
• What is the significance of using hydrochloric acid in the setup?

  It produces 1 mole per dm³ of H+ ions
• How does sulfuric acid differ from hydrochloric acid in terms of H+ ion concentration?

  It produces two H+ ions per molecule
• What is the electrochemical series?

  A table of half cell reactions and potentials
• How are half cell reactions displayed in the electrochemical series?

  In reduced form with electrons included
• What does a positive value in the electrochemical series indicate?

  It indicates a strong tendency to gain electrons
• What is oxidation in terms of electron transfer?

  Loss of electrons