Exploring Electrochemistry Concepts

What is an electrochemical cell and its components?

• An electrochemical cell consists of two electrodes (anode and cathode), an electrolyte, and a separator.

• An electrochemical cell is made up of a resistor and a capacitor.

• An electrochemical cell has only one type of electrolyte.

• A battery consists of a single electrode and a conductor.

Explain the difference between galvanic and electrolytic cells.

• Galvanic cells generate electricity from spontaneous reactions; electrolytic cells require electricity to drive non-spontaneous reactions.

• Galvanic cells convert chemical energy into thermal energy; electrolytic cells convert thermal energy into chemical energy.

• Galvanic cells require electricity to operate; electrolytic cells generate electricity spontaneously.

• Galvanic cells are used in batteries; electrolytic cells are used in light bulbs.

What is 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 irrelevant in electrochemistry.

• The Nernst equation is used to calculate reaction rates.

• The Nernst equation is 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 of painting surfaces.

• Electrolysis is used in various applications including electroplating, metal extraction, water splitting for hydrogen production, and the purification of metals.

• Electrolysis is only applicable in the textile industry.

What are redox reactions and how do they occur?

• Redox reactions do not involve any changes in oxidation states.

• Redox reactions are chemical reactions where one substance is oxidized and another is reduced, involving the transfer of electrons.

• Redox reactions are limited to reactions in acidic solutions only.

• Redox reactions only involve the formation of new compounds without electron transfer.

Define standard electrode potential and its importance.

• Standard electrode potential is irrelevant to electrochemical cells.

• Standard electrode potential measures the temperature of a chemical reaction.

• Standard electrode potential is the voltage of a battery under load.

• Standard electrode potential is a measure of the potential of a reversible electrode at standard conditions, crucial for predicting redox reaction feasibility and calculating cell potentials.

How do you calculate the cell potential of an electrochemical cell?

• E_cell = E°_cell + (RT/nF) * ln(Q)

• E_cell = E°_cell - (RT/nF) * ln(Q)

• E_cell = E°_cell + (nF/RT) * ln(Q)

• E_cell = E°_cell - (nF/RT) * ln(Q)

What factors affect the rate of electrolysis?

• Type of light used during the process

• Time of day when electrolysis is performed

• Factors affecting the rate of electrolysis include electrolyte type, concentration, temperature, electrode surface area, applied voltage, and electrode material.

• Size of the container holding the electrolyte

Explain the role of electrodes in electrochemical cells.

• Electrodes facilitate oxidation and reduction reactions, generating electric current in electrochemical cells.

• Electrodes prevent chemical reactions from occurring.

• Electrodes are used to store energy in batteries.

• Electrodes only serve as connectors in circuits.

What is the significance of the salt bridge in a galvanic cell?

• The salt bridge acts as a barrier to stop electron flow.

• The salt bridge is used to generate heat in the cell.

• The salt bridge prevents ion flow to maintain charge separation.

• The salt bridge allows ion flow to maintain charge balance and enables continuous electron flow.