5.4.2 Electrochemical cells

• What is an electrochemical cell defined as?

  A device converting chemical energy into electrical energy
• What process occurs at the cathode in an electrochemical cell?

  Reduction
• What is the role of the salt bridge in an electrochemical cell?

  Maintains electrical neutrality
• What type of reactions are essential for the functioning of an electrochemical cell?

  Redox reactions
• The anode is the electrode where oxidation occurs, releasing electrons
• The electrolyte in an electrochemical cell allows the flow of electrons between the anode and cathode.

  False
• In an electrochemical cell, the oxidation reaction occurs at the anode
• Steps in the operation of an electrochemical cell

  1️⃣ Oxidation at the anode releases electrons

  2️⃣ Electrons flow to the cathode

  3️⃣ Reduction at the cathode accepts electrons

  4️⃣ Ions flow through the salt bridge to maintain neutrality
• In a zinc-copper cell, the electrolyte enables Zn²⁺ ions to move away from the anode
• What is an electrochemical cell?

  A device converting chemical energy to electrical energy
• What is the function of the anode in an electrochemical cell?

  Releases electrons
• What is the role of the electrolyte in an electrochemical cell?

  Enables ion flow
• Match the electrode process with its description:

  Anode ↔️ Releases electrons during oxidation

  Cathode ↔️ Accepts electrons during reduction
• What is the primary function of the electrolyte in an electrochemical cell?

  Allows ion flow
• In a zinc-copper electrochemical cell, the electrolyte enables Zn²⁺ ions to move away from the anode
• Standard electrode potential is measured relative to the standard hydrogen electrode.


  True
• What condition is necessary for a redox reaction to be spontaneous in an electrochemical cell?

  Positive potential difference
• Standard electrode potential is measured relative to the standard hydrogen
• A higher temperature increases the standard electrode potential.

  False
• What does a positive difference in standard electrode potentials between the anode and cathode indicate?

  Spontaneous reaction
• The cell potential of an electrochemical cell is the difference between the standard electrode potentials of the cathode and the anode
• If the cell potential is negative, the reaction is non-spontaneous.


  True
• The standard electrode potential of $Zn^{2 + } / Zn$ is -0.76 V
• What is the primary function of the electrolyte in an electrochemical cell?

  Allows ion flow
• What type of reaction occurs at the anode of an electrochemical cell?

  Oxidation
• Match the component of an electrochemical cell with its description:

  Anode ↔️ Electrode where oxidation occurs

  Cathode ↔️ Electrode where reduction occurs

  Electrolyte ↔️ Solution allowing ion flow

  Salt bridge ↔️ Connects half-cells to maintain neutrality
• What is the function of the cathode in an electrochemical cell?

  Accepts electrons
• The components of an electrochemical cell facilitate the conversion of chemical energy into electrical energy.


  True
• The electrical current in an electrochemical cell is generated by the flow of electrons
• Ion flow in the electrolyte facilitates continuous electron transfer through the electrochemical cell.


  True
• In which direction do electrons flow in an electrochemical cell?

  Anode to cathode
• A higher temperature in an electrochemical cell decreases the standard electrode potential
• Match the factor affecting standard electrode potential with its effect:

  Ion concentration ↔️ Higher concentration increases potential

  Temperature ↔️ Higher temperature decreases potential

  Pressure ↔️ Higher pressure increases potential
• What effect does a higher concentration of ions have on the standard electrode potential?

  Increases it
• Higher pressure on the electrochemical cell increases the standard electrode potential
• Steps in calculating cell potential using standard electrode potentials

  1️⃣ Identify the cathode and anode

  2️⃣ Determine the standard electrode potentials for each

  3️⃣ Subtract the anode potential from the cathode potential
• What is the formula for calculating cell potential?

  $E_{cell} =$$E_{cathode} - E_{anode}$
• What is the standard electrode potential of $Cu^{2 + } / Cu$?


  +0.34 V
• Match the electrochemical cell components with their descriptions:

  Anode ↔️ Where oxidation occurs

  Cathode ↔️ Where reduction occurs

  Electrolyte ↔️ Allows ion flow

  Salt bridge ↔️ Maintains electrical neutrality
• The anode releases electrons, causing oxidation.


  True