Electrochemical Cells Overview

A device that converts chemical energy into electrical energy and vice versa. It consists of two electrodes immersed in one or more suitable electrolytes.

Electrolytes are the medium that facilitates the flow of ions between electrodes.

<p>Oxidation and reduction reactions happen in separate containers that are not in direct contact with each other.</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

<p>negative</p> Signup and view all the answers

<p>The salt bridge completes the circuit and allows ions to pass between the two half cells. It prevents intermixing of the solutions and helps maintain electrical neutrality.</p> Signup and view all the answers

<p>Electrons flow from the anode to the cathode, while electric current flows from the cathode to the anode.</p> Signup and view all the answers

<p>The vertical line (/) or semicolon (;) separates the metal or solid phase from the electrolyte (or cation of the electrolyte) in the half-cell representation.</p> Signup and view all the answers

<p>The double line (//) indicates the salt bridge that separates the two half cells of the electrochemical cell.</p> Signup and view all the answers

<p>All of the above (D)</p> Signup and view all the answers

<p>EMF or cell potential is the difference in electrode potential between the two electrodes in an electrochemical cell.</p> Signup and view all the answers

<p>EMF is expressed in volts (V).</p> Signup and view all the answers

<p>Ecell = Ecathode - Eanode</p> Signup and view all the answers

<p>It is an arrangement of elements ordered by their increasing reduction potential values. It is also known as the activity series.</p> Signup and view all the answers

<p>Determining the pH of a solution (A)</p> Signup and view all the answers

<p>The standard electrode potential refers to the electrode potential of a half-cell under standard conditions (1M concentration of ions, 298 K, and 1 atm pressure).</p> Signup and view all the answers

<p>The Nernst equation is a mathematical expression used to calculate the electrode potential of a cell under non-standard conditions. It relates the electrode potential to the standard electrode potential, the concentration of ions, and the temperature of the cell.</p> Signup and view all the answers

<p>The equilibrium constant (Kc) is a measure of the relative amounts of reactants and products at equilibrium, providing insight into the extent to which a reaction proceeds toward completion under given conditions.</p> Signup and view all the answers

<p>The Nernst equation relates the standard cell potential (E°cell) to the equilibrium constant (Kc) by providing a means to calculate the cell potential under non-standard conditions and relate this potential to the equilibrium position of the reaction.</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>It is used to calculate the cell potential of a cell under non-standard conditions, allowing chemists to predict the direction and extent of electrochemical reactions under various conditions.</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

A device that transforms chemical energy into electrical energy and vice versa. It consists of two electrodes immersed in an electrolyte.

The electrode where oxidation occurs. Electrons flow from the anode to the cathode.

The electrode where reduction occurs. It receives electrons from the anode.

A substance that allows ions to flow between electrodes in an electrochemical cell.

A chemical reaction where an atom, molecule, or ion loses electrons. It is characterized by an increase in oxidation state.

A chemical reaction where an atom, molecule, or ion gains electrons. It is characterized by a decrease in oxidation state.

An electrochemical cell that produces electrical energy from chemical reactions. The reactions are spontaneous.

An electrochemical cell that uses electrical energy to drive a non-spontaneous chemical reaction.

A simple galvanic cell where a zinc rod is dipped in a zinc sulfate solution and a copper rod is dipped in a copper sulfate solution. Electrons flow from zinc to copper.

In a galvanic cell, the anode is the negative terminal where oxidation takes place. The oxidation half-cell is the part where oxidation occurs.

In a galvanic cell, the cathode is the positive terminal where reduction takes place. The reduction half-cell is the part where reduction occurs.

In a galvanic cell, electrons flow from the anode (negative terminal) to the cathode (positive terminal).

A component in a galvanic cell that connects the two half cells, allowing ions to pass between them. It prevents intermixing of solutions and maintains electrical neutrality.

A shorthand notation representing the components of an electrochemical cell. The anode is on the left, the cathode on the right, separated by a double line representing the salt bridge.

The potential difference between an electrode and its electrolyte solution. It depends on the nature of the metal, ion concentration, and temperature.

The potential difference between the two electrodes in an electrochemical cell. It is expressed in volts.

A list of elements arranged in order of increasing reduction potential values. It is also known as the activity series.

Metals higher in the electrochemical series are stronger reducing agents, while those lower are stronger oxidizing agents. The series helps predict the spontaneity of reactions.

A formula used to calculate the electrode potential of a half-cell. It takes into account the standard electrode potential, concentration of ions, and temperature.

The electrode potential of an electrode under standard conditions: 1 M concentration, 298 K temperature, 1 atm pressure for gases.

At equilibrium, the cell reaction reaches a state where the cell potential is zero (E = 0), and the free energy change for the reaction is also zero (ΔG = 0).

A constant that expresses the ratio of products to reactants at equilibrium, indicating the extent to which a reaction proceeds to completion.

The Nernst equation can be used to calculate the equilibrium constant (K) of a reaction using the standard cell potential (E°) and the number of electrons transferred (n).

Using the Nernst equation, one can calculate the concentration of an ionic species in a cell if the concentration of the other species and the cell potential are known.

The Nernst equation can be used to determine the pH of a solution in an electrochemical cell by relating the cell potential, standard cell potential, and the concentration of hydrogen ions.

The electrochemical cell provides a means to measure the pH of a solution by relating the cell potential to the concentration of hydrogen ions.

The Nernst equation, used to calculate electrode potential, considers the influence of ion concentration on the cell potential by measuring the deviation from standard electrode potential.

A cell that uses the difference in concentration of a particular ion between two compartments to generate an electric potential.

A cell that uses the difference in partial pressure of a gas between two compartments to generate an electric potential.

An electrochemical cell where the electrode and electrolyte are in direct contact. It simplifies the setup and eliminates the need for a salt bridge.