Electrochemistry Test

What is an electrochemical cell?

• A device that generates electrical energy through chemical reactions.

• A type of solar panel

• A tool for measuring temperature

• A device that uses wind energy to produce electricity

Explain the difference between galvanic cells and electrolytic cells.

• Galvanic cells and electrolytic cells both use electricity to drive non-spontaneous redox reactions.

• Galvanic cells and electrolytic cells both generate electricity from spontaneous redox reactions.

• Galvanic cells use electricity to drive non-spontaneous redox reactions, while electrolytic cells generate electricity from spontaneous redox reactions.

• Galvanic cells generate electricity from spontaneous redox reactions, while electrolytic cells use electricity to drive non-spontaneous redox reactions.

Define oxidation and reduction in the context of redox reactions.

• Oxidation is the combination of a substance with oxygen, while reduction is the removal of oxygen from a substance.

• Oxidation is the loss of electrons or an increase in oxidation state, while reduction is the gain of electrons or a decrease in oxidation state.

• Oxidation is the process of reducing the oxidation state, while reduction is the process of increasing the oxidation state.

• Oxidation is the gain of electrons or an increase in oxidation state, while reduction is the loss of electrons or a decrease in oxidation state.

What is the purpose of a salt bridge in an electrochemical cell?

• To regulate the temperature within the cell

• To increase the voltage output of the cell

• To maintain electrical neutrality and allow the flow of ions between the two half-cells.

• To prevent the flow of electrons between the two half-cells

Describe how a voltaic cell generates electricity.

• A voltaic cell generates electricity by converting heat energy directly into electrical energy.

• A voltaic cell generates electricity through a redox reaction that occurs between two half-cells.

• A voltaic cell generates electricity through gravitational force.

• A voltaic cell generates electricity by emitting light energy.

What is the standard hydrogen electrode and why is it important in electrochemistry?

• The standard hydrogen electrode is only used in theoretical calculations and not practical applications.

• The standard hydrogen electrode is a reference electrode used in electrochemistry to measure the standard electrode potential of other half-cells.

• The standard hydrogen electrode is used to generate electricity in batteries.

• It is important in electrochemistry because it is a source of hydrogen gas.

How are cell potentials related to the spontaneity of redox reactions?

• Cell potentials are related to the rate of redox reactions

• Cell potentials are not related to the spontaneity of redox reactions

• Cell potentials are inversely related to the spontaneity of redox reactions

• Cell potentials are related to the spontaneity of redox reactions through the Gibbs free energy change (ΔG). If the cell potential (E°cell) is positive, the reaction is spontaneous (ΔG < 0) and vice versa.

Explain the terms anode and cathode in an electrochemical cell.

• The anode is positively charged, and the cathode is negatively charged.

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

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

• The anode is where electrons are gained, and the cathode is where electrons are lost.

What is Faraday's law of electrolysis?

• The amount of chemical change produced by current flowing through an electrolytic cell is proportional to the quantity of electricity passed through the cell.

• The amount of chemical change produced by current flowing through an electrolytic cell is inversely proportional to the quantity of electricity passed through the cell.

• Faraday's law of electrolysis only applies to solid conductors.

• Faraday's law of electrolysis states that the chemical change produced is not related to the quantity of electricity passed through the cell.

Discuss the applications of electrochemistry in everyday life.

• Batteries, electrolysis, electroplating, corrosion prevention, sensors

• Corrosion prevention in clothing

• Electroplating in gardening tools

• Electrolysis in cooking food