WorksheetsUnderstanding Electrochemical Cells
Total questions: 10
Worksheet time: 5mins
What is an electrochemical cell?
An electrochemical cell is a device that converts chemical energy into electrical energy.
A device that stores electrical energy for later use.
A type of battery that only works with solar energy.
A machine that generates heat from chemical reactions.
Describe the difference between galvanic and electrolytic cells.
Galvanic cells require electricity to operate; electrolytic cells generate electricity.
Galvanic cells involve chemical reactions only; electrolytic cells involve physical changes only.
Galvanic cells are used in batteries; electrolytic cells are used in light bulbs.
Galvanic cells generate electricity from spontaneous reactions; electrolytic cells require electricity to drive non-spontaneous reactions.
What role do electrodes play in an electrochemical cell?
Electrodes facilitate electron transfer in an electrochemical cell, with the anode enabling oxidation and the cathode enabling reduction.
Electrodes generate heat to facilitate chemical reactions.
Electrodes store energy in an electrochemical cell.
Electrodes are used to insulate the cell from external currents.
Explain the function of the salt bridge in a galvanic cell.
The salt bridge maintains electrical neutrality and allows ion flow between half-cells in a galvanic cell.
The salt bridge prevents ion flow between half-cells.
The salt bridge generates electricity in the galvanic cell.
The salt bridge acts as a barrier to stop electron movement.
What is the standard electrode potential?
The standard electrode potential is the mass of the reactants involved in a reaction.
The standard electrode potential is the voltage associated with a half-cell reaction at standard conditions.
The standard electrode potential measures the concentration of ions in a solution.
The standard electrode potential is the temperature at which a reaction occurs.
How do you calculate the cell potential of an electrochemical cell?
E_cell = E°_cell - (nF/RT) ln(Q)
E_cell = E°_cell + (RT/nF) ln(Q)
E_cell = E°_cell - (RT/nF) ln(Q)
E_cell = E°_cell + (nF/RT) ln(Q)
What is oxidation and reduction in the context of electrochemistry?
Oxidation is the loss of electrons; reduction is the gain of electrons.
Oxidation involves the increase of mass; reduction involves the decrease of mass.
Oxidation is the transfer of heat; reduction is the transfer of light.
Oxidation is the gain of protons; reduction is the loss of protons.
Describe the process of electrolysis and its applications.
Electrolysis is a method of painting surfaces.
Electrolysis is primarily used for cooking food.
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 in water splitting for hydrogen fuel production.
What factors affect the rate of electrochemical reactions?
Temperature, concentration, surface area, electrolyte nature, and catalysts.
Humidity levels
Type of metal used
Ambient light conditions
How can electrochemical cells be used in real-world applications?
Electrochemical cells are used for cooking food.
Electrochemical cells are used in water filtration systems.
Electrochemical cells are used in batteries, fuel cells, and electroplating.
Electrochemical cells are used for air conditioning systems.
