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Electrochemistry is primarily concerned with the study of nuclear reactions and particle physics.
Answer: False
Electrochemistry fundamentally investigates the relationship between electrical potential and chemical change, specifically involving electron transfer through circuits, not the study of nuclear reactions or particle physics.
In electrochemical reactions, electrons are transferred directly between reacting species without an external circuit.
Answer: False
Electrochemical reactions are characterized by the transfer of electrons via an external electric circuit, distinguishing them from conventional chemical reactions where direct transfer might occur.
The term 'redox' refers to reactions involving the transfer of heat between substances.
Answer: False
The term 'redox' is derived from 'reduction' and 'oxidation,' referring to reactions involving the transfer of electrons.
In a redox reaction, a reducing agent accepts electrons and is itself reduced.
Answer: False
A reducing agent donates electrons and is itself oxidized; an oxidizing agent accepts electrons and is itself reduced.
What is the fundamental definition of electrochemistry according to the provided text?
Answer: The relationship between electrical potential difference and identifiable chemical change.
Electrochemistry is defined as the branch of physical chemistry that investigates the relationship between electrical potential difference and discernible chemical transformations, specifically concerning electron transfer.
How are electrochemical reactions fundamentally different from conventional chemical reactions?
Answer: In electrochemical reactions, electrons are transferred via an external electric circuit, not directly between species.
Electrochemical reactions are fundamentally distinguished from conventional chemical reactions by their mechanism of electron transfer, which occurs via an external electric circuit.
What does the term 'redox' refer to in electrochemistry?
Answer: Reactions involving the transfer of electrons between species.
The term 'redox' is a portmanteau of 'reduction' and 'oxidation,' denoting chemical reactions characterized by the transfer of electrons between reacting species.
In a redox reaction, what is the role of a reducing agent?
Answer: It donates electrons and is itself oxidized.
In a redox reaction, a reducing agent functions by donating electrons, thereby undergoing oxidation itself.
William Gilbert, known as the 'Father of Magnetism,' dedicated his research primarily to understanding electrical phenomena in the 16th century.
Answer: False
William Gilbert's extensive work focused primarily on magnetism, although his investigations also laid early groundwork for understanding electrical phenomena.
Otto von Guericke invented the first electric generator in 1663, which used a sulfur ball to produce static electricity.
Answer: True
In 1663, Otto von Guericke constructed the first electric generator, utilizing a sulfur ball to produce static electricity through friction.
Charles François de Cisternay du Fay proposed that static electricity consisted of a single type of electrical fluid.
Answer: False
Charles François de Cisternay du Fay proposed the 'two-fluid theory,' suggesting static electricity comprised two types: vitreous and resinous.
Luigi Galvani's experiments with frog legs led him to propose the concept of 'animal electricity' in biological tissues.
Answer: True
Luigi Galvani's experiments with frog legs were pivotal in his proposal of 'animal electricity' as an intrinsic property of biological tissues.
Alessandro Volta agreed with Galvani's 'animal electricity' theory and used it to invent the first practical battery.
Answer: False
Alessandro Volta disagreed with Galvani's theory, proposing instead that electrical effects arose from the contact of dissimilar metals, leading to his invention of the Voltaic pile.
What significant contribution did Otto von Guericke make in 1663?
Answer: He created the first electric generator using a sulfur ball.
In 1663, Otto von Guericke constructed the first electric generator, an apparatus featuring a sulfur ball designed to produce static electricity.
Charles François de Cisternay du Fay's 'two-fluid theory' suggested that static electricity consisted of which two types?
Answer: Vitreous and Resinous
Charles François de Cisternay du Fay's 'two-fluid theory' proposed that static electricity comprised two types: 'vitreous' and 'resinous'.
What was Alessandro Volta's key disagreement with Luigi Galvani's findings?
Answer: Volta proposed that electrical effects were due to the contact between different metals, not 'animal electricity'.
Alessandro Volta dissented from Galvani's 'animal electricity' hypothesis, contending that the observed electrical effects stemmed from the contact between dissimilar metals.
Michael Faraday and John Frederic Daniell are widely recognized as the pioneers who established the field of electrochemistry.
Answer: True
John Frederic Daniell and Michael Faraday are indeed credited as foundational figures in establishing the field of electrochemistry through their extensive research and contributions.
In 1800, William Nicholson and Johann Wilhelm Ritter used Volta's battery to synthesize hydrogen and oxygen from water.
Answer: True
William Nicholson and Johann Wilhelm Ritter demonstrated the electrolysis of water into hydrogen and oxygen in 1800, utilizing the current generated by Volta's battery.
Hans Christian Ørsted's 1820 discovery established a link between magnetism and static electricity.
Answer: False
Hans Christian Ørsted's 1820 discovery established a link between electric currents and magnetism, not static electricity.
Georg Ohm's 1827 work primarily focused on the chemical properties of electrolytes.
Answer: False
Georg Ohm's seminal 1827 work focused on the relationship between voltage, current, and resistance in electrical circuits.
Michael Faraday coined the terms 'electrolyte' and 'electrolysis' during his 19th-century research.
Answer: True
Michael Faraday introduced fundamental terminology to the field, including the terms 'electrolyte' and 'electrolysis'.
John Daniell's 1836 primary cell invention aimed to increase the rate of polarization.
Answer: False
John Daniell's 1836 primary cell invention was designed to solve the problem of polarization in electrochemical cells.
Svante Arrhenius proposed in 1884 that electrolytes conduct electricity because they break down into neutral molecules when dissolved in water.
Answer: False
Svante Arrhenius proposed that electrolytes conduct electricity because they dissociate into electrically charged ions, not neutral molecules.
Robert Andrews Millikan's experiments starting in 1909 were designed to measure the mass of the electron.
Answer: False
Robert Andrews Millikan's famous oil drop experiment was designed to measure the fundamental charge of a single electron, not its mass.
Faraday's first law of electrolysis states that the mass deposited is proportional to the chemical equivalent weight.
Answer: False
Faraday's first law states that the mass deposited is proportional to the quantity of electricity passed. The second law relates quantities to equivalent weights.
Faraday's second law of electrolysis relates the quantities of different substances liberated by the same amount of electricity to their respective chemical equivalent weights.
Answer: True
Faraday's second law indeed establishes that the quantities of different substances produced by the same amount of electricity are proportional to their chemical equivalent weights.
Michael Faraday is credited with coining the term 'electrolysis'.
Answer: True
Michael Faraday is credited with coining the term 'electrolysis' during his pioneering research in electrochemistry.
Who are credited as the founders of the field of electrochemistry?
Answer: John Frederic Daniell and Michael Faraday
John Frederic Daniell and Michael Faraday are recognized as the seminal figures who established the field of electrochemistry through their extensive experimental work and theoretical contributions.
What groundbreaking electrochemical process did William Nicholson and Johann Wilhelm Ritter demonstrate in 1800?
Answer: The decomposition of water into hydrogen and oxygen using Volta's battery.
In 1800, William Nicholson and Johann Wilhelm Ritter achieved a landmark demonstration by decomposing water into hydrogen and oxygen via electrolysis, powered by the current from Volta's battery.
Hans Christian Ørsted's discovery in 1820 established a crucial link between which two fundamental forces?
Answer: Electricity and Magnetism
Hans Christian Ørsted's 1820 discovery revealed the magnetic effect of electric currents, thereby establishing a fundamental linkage between electricity and magnetism.
What fundamental law relating voltage, current, and resistance was published by Georg Ohm in 1827?
Answer: Ohm's Law
In 1827, Georg Ohm published his seminal work which included his eponymous law, quantifying the relationship between voltage, current, and resistance in electrical circuits.
Which of the following terms was coined by Michael Faraday?
Answer: Electrolyte and Electrolysis
Michael Faraday made substantial contributions to the lexicon of electrochemistry, notably by coining fundamental terms such as 'electrolyte' and 'electrolysis'.
What problem did John Daniell's primary cell invention in 1836 address?
Answer: The issue of polarization in electrochemical cells.
John Daniell's invention of a primary cell in 1836 was designed to overcome the problem of polarization, which hindered the performance of earlier electrochemical cells.
Svante Arrhenius's 1884 thesis proposed that electrolytes, when dissolved in water, dissociate into:
Answer: Electrically charged positive and negative ions
Svante Arrhenius proposed that electrolytes, upon dissolution in water, dissociate into positively and negatively charged ions, thereby accounting for their electrical conductivity.
Robert Andrews Millikan's famous oil drop experiment was designed to measure what fundamental physical quantity?
Answer: The charge of a single electron
Robert Andrews Millikan's renowned oil drop experiment was meticulously designed to ascertain the precise electric charge of a single electron.
Faraday's first law of electrolysis establishes a direct proportionality between the mass of a substance deposited and:
Answer: The quantity of electricity passed through the cell.
Faraday's first law of electrolysis posits that the mass of a substance deposited or liberated at an electrode is directly proportional to the quantity of electric charge passed through the electrolytic cell.
Faraday's second law of electrolysis relates the quantities of different substances liberated by the same amount of electricity to their:
Answer: Chemical equivalent weights
Faraday's second law of electrolysis states that the quantities of different substances liberated or deposited by a given amount of electricity are proportional to their respective chemical equivalent weights.
The Nernst equation allows for the calculation of cell potential under standard conditions only.
Answer: False
The Nernst equation is specifically used to calculate cell potential under non-standard conditions, relating it to reactant and product concentrations.
Galvanic cells generate electricity from spontaneous redox reactions, while electrolytic cells use electricity to drive non-spontaneous reactions.
Answer: True
This statement accurately distinguishes between galvanic cells, which produce electricity from spontaneous reactions, and electrolytic cells, which use electricity to drive non-spontaneous reactions.
The anode is the electrode where reduction occurs in an electrochemical cell.
Answer: False
The anode is defined as the electrode where oxidation occurs; reduction occurs at the cathode.
In a Daniell cell, zinc metal is reduced at the cathode.
Answer: False
In a Daniell cell, zinc metal is oxidized at the anode (Zn → Zn2+ + 2e-), while copper ions are reduced at the cathode (Cu2+ + 2e- → Cu).
The Standard Hydrogen Electrode (SHE) has a standard electrode potential of 1 volt by definition.
Answer: False
By definition, the standard electrode potential of the Standard Hydrogen Electrode (SHE) is 0 volts, serving as the reference point.
The standard cell potential (E°cell) is calculated by adding the standard electrode potentials of the cathode and anode.
Answer: False
The standard cell potential is calculated by subtracting the standard electrode potential of the anode from that of the cathode (E°cell = E°cathode - E°anode).
A negative change in Gibbs free energy (ΔG) indicates a non-spontaneous redox reaction in an electrochemical cell.
Answer: False
A negative change in Gibbs free energy (ΔG) signifies a spontaneous reaction, which corresponds to a positive cell potential capable of generating electrical energy.
Concentration cells generate electricity because the difference in concentration drives a spontaneous reaction.
Answer: True
Concentration cells operate based on the principle that a difference in ion concentration between two half-cells drives a spontaneous electrochemical reaction.
The Nernst equation is primarily used to understand the principles of magnetism in biological systems.
Answer: False
The Nernst equation is primarily used to calculate cell potentials based on ion concentrations and is relevant to biological electrical phenomena, not magnetism.
The diagram showing Zn(s) | Zn2+ (1 M) || Cu2+ (1 M) | Cu(s) illustrates a concentration cell.
Answer: False
This diagram represents a standard Daniell cell, not a concentration cell, as it involves different electrode materials and standard concentrations.
A concentration cell, like Cu(s) | Cu2+ (0.05 M) || Cu2+ (2.0 M) | Cu(s), generates electricity due to differences in electrode material.
Answer: False
Concentration cells generate electricity due to differences in electrolyte concentration, not electrode material, when the electrodes are identical.
What is the primary purpose of the Nernst equation in electrochemistry?
Answer: To relate the cell potential to the concentrations of reactants and products under non-standard conditions.
The Nernst equation serves to calculate the cell potential under non-standard conditions, quantifying the influence of reactant and product concentrations on the cell's electromotive force.
Which type of electrochemical cell produces electricity from spontaneous redox reactions?
Answer: Galvanic (or Voltaic) cell
Galvanic (or Voltaic) cells are designed to generate electrical energy from spontaneous redox reactions.
In an electrochemical cell, oxidation occurs at which electrode?
Answer: The anode
Within an electrochemical cell, the anode is defined as the electrode where oxidation (the loss of electrons) takes place.
What are the half-reactions occurring at the electrodes in a standard Daniell cell?
Answer: Anode: Zn(s) → Zn2+ + 2e-; Cathode: Cu2+ + 2e- → Cu(s)
In a standard Daniell cell, the anode reaction involves the oxidation of zinc (Zn(s) → Zn2+(aq) + 2e-), and the cathode reaction involves the reduction of copper ions (Cu2+(aq) + 2e- → Cu(s)).
What is the standard electrode potential of the Standard Hydrogen Electrode (SHE)?
Answer: 0.00 V
By definition, the standard electrode potential of the Standard Hydrogen Electrode (SHE) is assigned a value of zero volts, serving as the universal reference standard.
How is the standard cell potential (E°cell) calculated using standard electrode potentials?
Answer: E°cell = E°red (cathode) – E°red (anode)
The standard cell potential (E°cell) is quantitatively determined by subtracting the standard electrode potential of the anode from that of the cathode: E°cell = E°red (cathode) – E°red (anode).
A negative change in Gibbs free energy (ΔG) in an electrochemical cell indicates:
Answer: A spontaneous reaction capable of generating electrical energy.
A negative change in Gibbs free energy (ΔG) signifies a spontaneous reaction, which correlates with a positive cell potential, enabling the cell to perform electrical work.
The diagram Zn(s) | Zn2+ (1 M) || Cu2+ (1 M) | Cu(s) represents which type of electrochemical cell under standard conditions?
Answer: Daniell cell
The cell diagram Zn(s) | Zn2+ (1 M) || Cu2+ (1 M) | Cu(s) represents a standard Daniell cell, a type of galvanic cell.
What drives the electrochemical reaction in a concentration cell like Cu(s) | Cu2+ (0.05 M) || Cu2+ (2.0 M) | Cu(s)?
Answer: Difference in electrolyte concentrations.
In a concentration cell, the electrochemical potential is generated by the difference in electrolyte concentration between the two half-cells, driving the reaction towards equilibrium.
Electrolysis uses spontaneous redox reactions to generate electrical energy.
Answer: False
Electrolysis uses an external electrical energy source to drive non-spontaneous redox reactions, whereas galvanic cells use spontaneous reactions to generate electricity.
The electrolysis of molten sodium chloride primarily produces sodium hydroxide and chlorine gas.
Answer: False
The electrolysis of molten sodium chloride yields metallic sodium and chlorine gas, not sodium hydroxide.
An electrolyte is typically added during the electrolysis of water to decrease its electrical conductivity.
Answer: False
An electrolyte is added to water during electrolysis to increase its electrical conductivity, as pure water is a poor conductor.
The electrolysis of aqueous sodium chloride solution produces hydrogen gas at the cathode and chlorine gas at the anode.
Answer: True
The electrolysis of aqueous sodium chloride yields hydrogen gas at the cathode, chlorine gas at the anode, and sodium hydroxide in solution.
Electroplating relies on Faraday's laws to control the amount of metal deposited.
Answer: True
Faraday's laws are fundamental to electroplating, enabling precise control over the quantity and thickness of the deposited metal based on electrical parameters.
Overvoltage in electrolysis refers to the potential required to drive a reaction at a practical rate, beyond thermodynamic predictions.
Answer: True
Overvoltage is the excess potential required to overcome kinetic barriers and drive an electrolytic reaction at a practical rate, beyond what thermodynamics alone predicts.
The Chloralkali process involves the electrolysis of molten potassium chloride.
Answer: False
The Chloralkali process involves the electrolysis of aqueous sodium chloride, not molten potassium chloride.
What is electrolysis?
Answer: A process using an external electrical energy source to drive non-spontaneous redox reactions.
Electrolysis is defined as a process wherein an external source of electrical energy is employed to drive a non-spontaneous redox reaction, typically within an electrolytic cell.
What are the primary products of the electrolysis of molten sodium chloride?
Answer: Metallic sodium and gaseous chlorine
The electrolysis of molten sodium chloride, commonly performed in a Downs cell, yields metallic sodium and gaseous chlorine as its principal products.
Why is an electrolyte typically added during the electrolysis of water?
Answer: To increase the electrical conductivity of the water.
An electrolyte is typically added to water during electrolysis to enhance its electrical conductivity, as pure water exhibits very low conductivity.
Which of the following are the main products of the electrolysis of an aqueous sodium chloride solution?
Answer: Hydrogen gas, chlorine gas, and sodium hydroxide
Electrolysis of an aqueous sodium chloride solution characteristically yields hydrogen gas at the cathode, chlorine gas at the anode, and sodium hydroxide in the solution.
How is electroplating directly related to Faraday's laws?
Answer: Faraday's laws are used to determine the precise amount of metal to deposit.
Electroplating is directly governed by Faraday's laws, which enable the precise control of the deposited metal's mass and thickness by correlating it with the quantity of electricity applied.
What does the overvoltage effect in electrolysis refer to?
Answer: The extra potential needed to drive an electrolytic reaction at a practical rate beyond thermodynamics.
The overvoltage effect in electrolysis denotes the additional electrical potential required to achieve a practical reaction rate, exceeding thermodynamic predictions, often due to kinetic barriers.
What are the main products of the Chloralkali process?
Answer: Hydrogen gas, chlorine gas, and sodium hydroxide
The Chloralkali process, a major industrial method involving the electrolysis of aqueous sodium chloride, yields hydrogen gas, chlorine gas, and sodium hydroxide as its primary products.
Arne Tiselius developed a sophisticated apparatus for electrophoresis in 1937, a technique for separating charged molecules.
Answer: True
Arne Tiselius developed a sophisticated apparatus for electrophoresis in 1937, a technique crucial for separating charged molecules.
Corrosion is considered an electrochemical process involving oxidation at anodic sites and reduction at cathodic sites.
Answer: True
Corrosion is fundamentally an electrochemical process involving oxidation at anodic sites and reduction at cathodic sites on the metal surface.
Iron requires only oxygen, but not water, to undergo rusting.
Answer: False
Iron requires the presence of both oxygen and water to undergo the electrochemical process of rusting.
The presence of electrolytes like salt accelerates the rusting of iron by decreasing the conductivity of the solution.
Answer: False
Electrolytes like salt accelerate rusting by increasing the solution's conductivity, thereby facilitating the electrochemical circuit.
Metals like titanium and aluminum resist corrosion by forming a thick, porous oxide layer.
Answer: False
Titanium and aluminum resist corrosion by forming a thin, tightly adhering, passive oxide layer, not a thick, porous one.
Sacrificial anodes are used to protect a structure by corroding preferentially.
Answer: True
Sacrificial anodes, being more reactive, corrode preferentially, thereby protecting the primary structure from corrosion.
Fuel cells are an example of electrochemical energy storage devices.
Answer: False
Fuel cells are electrochemical energy conversion devices, not storage devices; batteries are typically considered energy storage devices.
Photosynthesis is considered an electrochemical process involving electron transfer steps.
Answer: True
Photosynthesis is fundamentally an electrochemical process, involving critical electron transfer steps in the conversion of light energy to chemical energy.
Which technique, developed by Arne Tiselius in 1937, is used to separate charged molecules?
Answer: Electrophoresis
Arne Tiselius developed a sophisticated apparatus for electrophoresis in 1937, a technique crucial for the separation of charged molecules.
What is the primary electrochemical perspective on corrosion?
Answer: An electrochemical process involving oxidation and reduction.
From an electrochemical perspective, corrosion is understood as a process wherein metals undergo reactions with their environment, typically involving oxidation and reduction.
What are the essential conditions required for iron to undergo rusting?
Answer: Exposure to both oxygen and water.
The process of iron rusting necessitates the simultaneous presence of both oxygen and water; these environmental factors are indispensable for the electrochemical corrosion mechanism to proceed.
Why does the presence of an electrolyte, like salt, accelerate the rusting of iron?
Answer: Salt increases the conductivity of the solution, facilitating the electrochemical circuit.
Electrolytes, such as dissolved salts, accelerate iron rusting by enhancing the electrical conductivity of the aqueous medium, thereby completing the electrochemical circuit required for corrosion.
How do metals like titanium and aluminum typically protect themselves from corrosion?
Answer: By forming a very thin, tightly adhering oxide layer that acts as a barrier.
Metals such as titanium and aluminum resist corrosion by forming a thin, adherent, and passivating oxide layer upon exposure to the atmosphere, which effectively impedes further environmental interaction.
What is the principle behind using sacrificial anodes to prevent corrosion?
Answer: A more reactive metal corrodes preferentially, protecting the main structure.
The principle of sacrificial anodes involves attaching a more electrochemically active metal that corrodes preferentially, thereby protecting the primary structure by forcing it to act as a cathode.
Which of the following is an example of an electrochemical energy conversion technology?
Answer: Fuel cell
Fuel cells are electrochemical energy conversion technologies that directly transform chemical energy into electrical energy.
How is photosynthesis described in relation to electrochemistry?
Answer: As an electrochemical process involving electron transfer.
Photosynthesis is fundamentally understood as an electrochemical process, involving critical electron transfer steps in the conversion of light energy to chemical energy.