IGCSE 11.3.8
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An electrochemical cell consists of two different metals submerged in an electrolyte such as an acid or salt solution. Electrons flow from the more reactive metal, creating a voltage. For example, in a zinc-copper cell, zinc releases electrons into the electrolyte more readily than copper, becoming the negative electrode. The electrons flow to the copper electrode.
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Chapter 20 Lecture- Electrochemistry
Let's balance this step-by-step using the half-reaction method:
Oxidation: Ag → Ag+
Reduction: 1/2O2 + H+ → H2O
Balanced half-reactions:
Ag → Ag+
1/2O2 + H+ → H2O
Overall balanced reaction:
1Ag + 1/2O2 + 1H+ → 1Ag+ + 1H2O
The correct coefficients are:
1, 1/2, 1, 1, 1
The answer is 1.
Electrochemistry
This document provides an overview of electrochemistry. It begins by defining electrochemistry as the study of chemical reactions at the interface of an electrode and electrolyte involving the interaction of electrical and chemical changes. The document then discusses the history and founders of electrochemistry, including Faraday's two laws of electrolysis. It explains key concepts such as oxidation-reduction reactions, balancing redox equations, and the Nernst equation. The document also covers applications including batteries, corrosion, electrolysis, and branches of electrochemistry like bioelectrochemistry and nanoelectrochemistry.
Fundamentals of Electrochemistry
Electrochemistry is Everywhere - Nearly every Industry and Institute needs Electrochemistry ! The fundamentals of Electrochemistry
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Electrolysis is the process of using direct electrical current to cause a non-spontaneous chemical reaction. During electrolysis, ions conduct electricity and move towards the electrode that attracts them. The key factors that determine the products of electrolysis include:
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IGCSE 11.3.3
The document discusses the reactivity and oxidation of zinc and copper. Zinc is described as a relatively reactive metal that readily gives away electrons to form zinc ions in solution. In contrast, copper is characterized as an unreactive metal that prefers to remain as copper metal and rarely donates electrons to form copper cations.
ELECTRICITY AND CHEMISTRY
1. Electrolysis is the process of using electricity to cause non-spontaneous chemical changes.
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The document provides information about electrolysis, including:
1) Electrolysis is the chemical effect of electricity on ionic compounds, causing them to break up into simpler substances like elements.
2) During electrolysis, ions move to electrodes of opposite charge where chemical reactions occur - non-metals form at the anode and metals or hydrogen form at the cathode.
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This document provides an overview of electrochemistry concepts including:
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The document describes a lab experiment comparing the reactions of different metals with hydrochloric acid. Students observed the reactions of zinc, magnesium, copper, and aluminum with HCl of varying concentrations. Zinc and magnesium reacted vigorously while copper did not react at all. The purpose was to model oxidation-reduction reactions and construct equations to summarize the single replacement reactions. Students analyzed the reactions in terms of atoms becoming ions, oxidation states changing, and the energy changes involved. Reactions that produced heat were determined to be exothermic.
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The document discusses conductivity (or specific conductance) of metal ions in solution, which is a measure of its ability to conduct electricity. It explains that conductivity is higher for strong electrolytes that nearly completely dissociate into ions in solution, while weak electrolytes only partially dissociate. Several factors influence conductivity, including the nature of the solute and solvent, concentration, and temperature. Conductivity measurements are used in various industrial applications like water treatment and leak detection.
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The document discusses electrolysis and the principles behind it. It explains that electrolysis involves passing electricity through an electrolyte, which causes chemical decomposition. Ions migrate to the electrodes and are discharged. Metals are formed at the cathode by reduction, while non-metals or oxygen form at the anode by oxidation. It provides examples of electrolysis such as molten salts like NaCl and aqueous solutions like copper sulfate. Factors affecting ion discharge are also discussed.
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2. Electromotive force (EMF) is the energy supplied by a source of electric power to drive a unit positive charge around a circuit. It is measured in volts and is the potential difference between the terminals of a cell when the circuit is open.
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Here are the identifications:
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A voltaic cell converts chemical energy to electrical energy using two different metals immersed in an electrolyte. The more electropositive metal becomes the negative terminal, releasing electrons that flow through an external circuit to the other metal, which acts as the positive terminal. For example, a zinc-copper voltaic cell uses zinc and copper plates in a dilute sulfuric acid electrolyte, with zinc dissolving as ions and electrons flowing to the copper where they combine with hydrogen ions to produce bubbles of hydrogen gas. Zinc is higher than copper in the electrochemical series, so it more easily releases electrons to power the flow of current.
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This document discusses different types of electrochemical cells including galvanic/voltaic cells which produce electrical energy from spontaneous reactions and electrolytic cells which require electrical energy for non-spontaneous reactions. It describes how voltaic cells work by separating the oxidation and reduction half reactions into two half cells connected by a salt bridge or porous disk to allow ion flow. Common examples discussed include copper-zinc voltaic cells, dry cells like flashlights, lead storage batteries in cars, and hydrogen-oxygen fuel cells.
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This document discusses different types of electrochemical cells including galvanic/voltaic cells which produce electrical energy from spontaneous reactions and electrolytic cells which require electrical energy for non-spontaneous reactions. It describes how voltaic cells work by separating the oxidation and reduction half reactions into two half cells connected by a salt bridge or porous disk to allow ion flow. Common examples discussed include copper-zinc voltaic cells, dry cells like flashlights, lead storage batteries in cars, and hydrogen-oxygen fuel cells.
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Electrolytes are substances that can conduct electricity in the molten or liquid state and undergo chemical changes. Electrolysis is a process where electrolytes are broken down into their constituent elements by passing electricity through them. During electrolysis, ions migrate to the oppositely charged electrodes. At the anode, ions lose electrons and form gases or dissolve. At the cathode, ions gain electrons and form solid elements. Examples of electrolysis of molten lead(II) bromide and lead(II) oxide are described through their half reactions at the anode and cathode and overall reactions.
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Lifts, cars, and other large electrical machines use high currents. Relays use an electromagnet to allow a small current in one circuit to control a large current in another circuit. This allows a small current to control whether a large current flows through another circuit by closing or opening a switch.
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The circuit for a door bell contains an electromagnet that pulls an armature towards it when the circuit is closed, causing a hammer to strike the bell and produce sound. The movement of the armature then breaks the circuit, allowing the hammer to return to its original position, and this sequence repeats to make the bell ring continuously whenever the door bell button is pressed.
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An electromagnet on a recycling plant conveyor belt is used to pick up and move metal cans. Electromagnets attract ferromagnetic metals like iron, nickel, and cobalt. Electromagnets have the advantage over permanent magnets in that their magnetic field can be switched on and off by controlling the electric current running through the magnet coils.
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The document presents results from an experiment investigating electromagnets. It shows that increasing the number of coils or the current in an electromagnet increases the number of drawing pins attracted. Graphs illustrate the direct relationship between the number of coils/current and the number of drawing pins attracted.
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An experiment was designed to investigate how changing the current and number of coils affects the strength of an electromagnet. The apparatus shown could be used by altering the current running through the coils or changing the number of coils wrapped around the iron core, then measuring the effect on the magnetic force produced. Results could show that increasing either the current or number of coils strengthens the electromagnet.
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IGCSE 11.3.8
- 2. Simple electrochemical cells An electrochemical cell consists of two metals of different reactivity dipped into an electrolyte.
- 3. Simple electrochemical cells An electrochemical cell consists of two metals of different reactivity dipped into an electrolyte. The electrolyte can be an acid, alkali or a solution of a salt.
- 4. Simple electrochemical cells An electrochemical cell consists of two metals of different reactivity dipped into an electrolyte. The electrolyte can be an acid, alkali or a solution of a salt. When connceted electrons will flow creating a voltage.
- 5. Half reactions The zinc is better at releasing electrons than copper. So zinc will be converted to zinc ions
- 6. Half reactions The zinc is better at releasing electrons than copper. So zinc will be converted to zinc ions Zn(s) Zn2+(aq) + 2e-
- 7. Half reactions The zinc is better at releasing electrons than copper. So zinc will be converted to zinc ions Zn(s) Zn2+(aq) + 2e- The zinc electrode becomes negative because of the number of electrons present. These electrons flow to the copper electrode.
- 8. Half reactions The zinc is better at releasing electrons than copper. So zinc will be converted to zinc ions Zn(s) Zn2+(aq) + 2e- The zinc electrode becomes negative because of the number of electrons present. These electrons flow to the copper electrode. At the other electrode the electrons are released and combine with hydrogen in the electrolyte.
- 9. Half reactions The zinc is better at releasing electrons than copper. So zinc will be converted to zinc ions Zn(s) Zn2+(aq) + 2e- The zinc electrode becomes negative because of the number of electrons present. These electrons flow to the copper electrode. At the other electrode the electrons are released and combine with hydrogen in the electrolyte. 2H+(aq) + 2e- H2(g)
- 10. Half reactions The zinc is better at releasing electrons than copper. So zinc will be converted to zinc ions Zn(s) Zn2+(aq) + 2e- The zinc electrode becomes negative because of the number of electrons present. These electrons flow to the copper electrode. At the other electrode the electrons are released and combine with hydrogen in the electrolyte. 2H+(aq) + 2e- H2(g)