Electrochemistry Quiz

What is a galvanic cell and how does it work?

• A galvanic cell is an electrochemical cell that converts chemical energy into electrical energy. It works by using redox reactions to generate a flow of electrons, which creates an electric current.

• A galvanic cell is a device that converts mechanical energy into electrical energy.

• A galvanic cell is a type of battery that uses solar energy to generate electricity.

• A galvanic cell is a type of fuel cell that uses hydrogen as the fuel.

Explain the role of anode and cathode in a galvanic cell.

• Anode and cathode play the roles of electron source and electron acceptor, respectively.

• Anode and cathode have the same function in a galvanic cell

• Anode and cathode are both positively charged

• Anode and cathode both act as electron acceptors

Describe the function of salt bridge in a galvanic cell.

• Maintains electrical neutrality and completes the circuit

• Generates electricity

• Increases the rate of corrosion

• Prevents the flow of electrons

What is an electrolytic cell and how does it differ from a galvanic cell?

• An electrolytic cell uses electrical energy to drive a non-spontaneous chemical reaction, while a galvanic cell uses a spontaneous chemical reaction to produce electrical energy.

• An electrolytic cell uses heat energy to drive a non-spontaneous chemical reaction, while a galvanic cell uses light energy to produce electrical energy.

• An electrolytic cell uses magnetic energy to drive a spontaneous chemical reaction, while a galvanic cell uses electrical energy to produce non-spontaneous chemical reaction.

• An electrolytic cell uses mechanical energy to drive a spontaneous chemical reaction, while a galvanic cell uses electrical energy to produce non-spontaneous chemical reaction.

Explain the process of electrolysis in an electrolytic cell.

• The process of electrolysis involves the use of electrical energy to drive a non-spontaneous chemical reaction.

• The process of electrolysis involves the use of mechanical energy to drive a spontaneous chemical reaction.

• Electrolysis is a process that does not involve the use of any external energy.

• Electrolysis occurs in a voltaic cell, not an electrolytic cell.

Differentiate between galvanic and electrolytic cells.

• Galvanic cells convert electrical energy into chemical energy, while electrolytic cells use chemical energy to drive a spontaneous reaction.

• Galvanic cells convert chemical energy into electrical energy, while electrolytic cells use electrical energy to drive a non-spontaneous chemical reaction.

• Galvanic cells use electrical energy to drive a non-spontaneous chemical reaction, while electrolytic cells convert chemical energy into electrical energy.

• Galvanic cells and electrolytic cells both convert chemical energy into electrical energy.

What are redox reactions and how are they related to electrochemistry?

• Redox reactions involve the transfer of protons between reactants, and electrochemistry is the study of these proton transfer processes.

• Redox reactions involve the transfer of photons between reactants, and electrochemistry is the study of these photon transfer processes.

• Redox reactions involve the transfer of electrons between reactants, and electrochemistry is the study of these electron transfer processes.

• Redox reactions involve the transfer of neutrons between reactants, and electrochemistry is the study of these neutron transfer processes.

Give an example of a redox reaction involving the transfer of electrons.

• Iron and water

• Aluminum and hydrochloric acid

• Copper and silver nitrate

• Sodium and potassium chloride

Explain the concept of electrode potential and its significance in electrochemistry.

• Electrode potential is the measure of the resistance of an electrode to oxidation or reduction.

• Electrode potential is the measure of the concentration of ions in a solution.

• Electrode potential is the measure of the temperature of an electrode during a redox reaction.

• Electrode potential is the measure of the tendency of an electrode to gain or lose electrons. It is significant in electrochemistry as it helps in determining the direction of the flow of electrons in a redox reaction and the feasibility of the reaction.

How is electrode potential related to the spontaneity of a redox reaction?

• Electrode potential is related to the spontaneity of a redox reaction through the concentration of the reactants

• Electrode potential is related to the spontaneity of a redox reaction through the Gibbs free energy change (ΔG).

• Electrode potential is related to the spontaneity of a redox reaction through the temperature of the reaction

• Electrode potential is related to the spontaneity of a redox reaction through the volume of the solution