3.1.11.1 Electrode Potentials

• Standard electrode potentials are measured under standard conditions.


  True
• Higher positive electrode potentials indicate a greater tendency to be reduced
• What is the potential of the standard hydrogen electrode (SHE) under standard conditions?

  0.00 V
• Higher positive electrode potentials mean a greater tendency to be reduced
• The SHE is used as a reference electrode to measure the electrode potentials of other half-cells.


  True
• Steps to measure electrode potentials using the SHE:

  1️⃣ Connect the half-cell of interest to the SHE using a salt bridge

  2️⃣ Use a voltmeter to measure the potential difference between the two half-cells
• Match the electrode potential value with its interpretation:

  Higher positive potential ↔️ Greater tendency to be reduced

  Lower potential ↔️ Greater tendency to be oxidized
• The standard hydrogen electrode (SHE) has a defined potential of 0.00 V under standard conditions.
• Electrode potentials are measured relative to the SHE under standard conditions.
• The standard hydrogen electrode (SHE) is assigned a potential of 0.00 V under standard conditions.

  True
• The standard hydrogen electrode (SHE) is assigned a potential of 0.00 V
• Components of the standard hydrogen electrode (SHE)

  1️⃣ Porous platinum coated disk

  2️⃣ Hydrogen gas at 1 atm

  3️⃣ 1 M solution of hydrogen ions

  4️⃣ Standard conditions of 298 K
• Lower electrode potentials indicate a stronger reducing agent.


  True
• Match the component of the SHE with its description:

  Platinum electrode ↔️ Porous platinum-coated disk

  Hydrogen gas ↔️ Bubbled through at 1 atm

  Electrolyte ↔️ 1 M solution of hydrogen ions
• The measured potential indicates the half-cell's tendency to be reduced or oxidized compared to the SHE.


  True
• Electrode potentials are always compared against the standard hydrogen electrode (SHE), which is assigned a potential of 0.00 V.
• Half-cells with lower electrode potentials are stronger reducing agents.


  True
• Steps to measure electrode potentials using the SHE:

  1️⃣ Connect the half-cell of interest to the SHE using a salt bridge

  2️⃣ Use a voltmeter to measure the potential difference between the two half-cells
• What does a higher positive electrode potential indicate compared to the SHE?

  Stronger oxidizing agent
• The cell potential is calculated by subtracting the E° of the oxidation half-reaction from the E° of the reduction half-reaction.
• Elevated temperatures always favor reduction in electrode reactions.

  False
• Electrode potentials measure the tendency of a half-cell to gain electrons
• Match the standard conditions with their values:

  Temperature ↔️ 298 K (25°C)

  Pressure ↔️ 1 atm (101.3 kPa)

  Concentration of ions ↔️ 1 M
• Lower electrode potentials indicate a stronger reducing agent.


  True
• The SHE is used to measure the electrode potentials of other half-cells.


  True
• The standard hydrogen electrode (SHE) is assigned an electrode potential of 0.00 V under standard conditions.
• Electrode potentials are measured relative to the SHE, which is assigned a potential of 0.00 V under standard conditions.
• The standard electrode potentials of half-cells indicate their relative reducing or oxidizing power compared to the SHE.
• Higher positive electrode potentials indicate stronger oxidizing agents.

  True
• Match the component of the SHE with its description:

  Platinum electrode ↔️ Porous platinum-coated disk

  Hydrogen gas ↔️ Bubbled through at 1 atm

  Electrolyte ↔️ 1 M solution of hydrogen ions
• Connect the half-cell of interest to the SHE using a salt bridge
• Match the electrode potential with its interpretation:

  Positive (+) ↔️ Greater tendency to be reduced

  Negative (-) ↔️ Greater tendency to be oxidized
• What is the cell potential of a cell with a reduction half-reaction of Cu²⁺ + 2e^- → Cu (E° = +0.34 V) and an oxidation half-reaction of Zn → Zn²⁺ + 2e^- (E° = -0.76 V)?

  +1.10 V
• What does the Nernst Equation quantify?

  Factors affecting electrode potentials
• The cell potential of an electrochemical cell is measured under standard conditions.

  True
• Higher ion concentrations generally shift the equilibrium towards reduction
• Faraday's constant (F) has a value of 96,485 C/mol.