Exploring Electrochemistry Concepts

What is the primary function of an electrochemical cell?

• To convert chemical energy into electrical energy.

• To generate chemical reactions without producing electricity.

• To store electrical energy for later use.

• To convert electrical energy into thermal energy.

Define the Nernst equation and its significance in electrochemistry.

• The Nernst equation is E = E° - (RT/nF)ln(Q) and is significant for calculating cell potentials under non-standard conditions.

• The Nernst equation is used to calculate reaction rates in chemical kinetics.

• The Nernst equation is irrelevant in determining cell voltages in electrochemical cells.

• The Nernst equation states that E = E° + (RT/nF)ln(Q) for standard conditions.

Describe the process of electrolysis and its applications.

• Electrolysis is primarily used for cooking food.

• Electrolysis is a method for increasing the temperature of metals.

• Electrolysis is only applicable in the textile industry.

• Electrolysis is used in various applications including electroplating, purification of metals, production of chemical compounds (like chlorine and hydrogen), and water splitting for hydrogen fuel.

What are redox reactions and how do they relate to electrochemistry?

• Redox reactions do not involve electron transfer.

• Electrochemistry is unrelated to chemical reactions.

• Redox reactions are processes involving electron transfer, crucial to electrochemistry, which studies their relationship with electrical energy.

• Redox reactions only occur in acidic solutions.

Explain the concept of standard electrode potentials.

• Standard electrode potentials measure the temperature of a reaction.

• Standard electrode potentials are the same as standard enthalpy changes.

• Standard electrode potentials are voltages that measure the tendency of a species to be reduced, relative to the standard hydrogen electrode.

• Standard electrode potentials are used to calculate the mass of a substance.

How do galvanic cells generate electrical energy?

• Galvanic cells generate energy through chemical heating processes.

• Galvanic cells generate electrical energy through spontaneous redox reactions that create a flow of electrons.

• Galvanic cells produce electricity by using solar energy.

• Galvanic cells create electrical energy by mechanical movement of parts.

What factors affect the voltage of an electrochemical cell?

• Concentration of reactants/products, temperature, electrode materials, and electrolyte type.

• Size of the electrochemical cell

• Duration of the experiment

• Type of light used in the experiment

Describe the role of the anode and cathode in an electrochemical cell.

• Both the anode and cathode are sites of oxidation.

• The anode is where reduction occurs and the cathode is where oxidation occurs.

• The anode is where oxidation occurs (loses electrons), and the cathode is where reduction occurs (gains electrons).

• The anode gains electrons while the cathode loses electrons.

What is the difference between a galvanic cell and an electrolytic cell?

• Galvanic cells use electricity; electrolytic cells generate electricity.

• Galvanic cells are used for electrolysis; electrolytic cells are used for power generation.

• Galvanic cells generate electricity; electrolytic cells consume electricity.

• Both galvanic and electrolytic cells generate electricity.

How can the Nernst equation be used to calculate cell potential under non-standard conditions?

• E = E° - (RT/nF) * ln(Q)

• E = E° - (nF/RT) * ln(Q)

• E = E° + (nF/RT) * ln(Q)

• E = E° + (RT/nF) * ln(Q)