Electrochemical Cells Quiz

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

The electrode where oxidation occurs. It is the negative terminal in a galvanic cell.

The electrode where reduction occurs. It is the positive terminal in a galvanic cell.

A medium that facilitates the flow of ions between electrodes in an electrochemical cell.

An electrochemical cell that produces electricity as a result of a spontaneous chemical reaction inside the cell, like a battery.

An electrochemical cell where electrical energy drives a non-spontaneous chemical reaction. It uses electricity to make a chemical change.

A simple galvanic cell consisting of a zinc electrode in a solution of zinc sulfate and a copper electrode in a solution of copper sulfate.

The process where electrons are lost, resulting in an increase in oxidation state. It occurs at the anode in a galvanic cell.

The process where electrons are gained, resulting in a decrease in oxidation state. It occurs at the cathode in a galvanic cell.

The half of an electrochemical cell where oxidation occurs.

The half of an electrochemical cell where reduction occurs.

The flow of electrons from the anode (negative terminal) to the cathode (positive terminal) in a galvanic cell.

A device that connects the two half-cells of a galvanic cell, allowing the flow of ions without mixing the solutions. It maintains electrical neutrality and prevents liquid junction potential.

A shorthand representation of an electrochemical cell, where the anode is on the left and the cathode on the right. The metal, electrolyte, and salt bridge are represented by specific symbols.

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

The potential difference between the two electrodes in an electrochemical cell. It is expressed in volts and represents the maximum electrical work the cell can do.

A table that lists elements in order of increasing reduction potential values. It helps predict the relative strength of oxidizing and reducing agents, reactivity, and feasibility of redox reactions.

The standard electrode potential of an electrode when the concentration of the electrolyte is 1 M, the temperature is 298 K, and the pressure of gaseous components is 1 atm.

An equation that relates the electrode potential of a half-cell to the standard electrode potential, temperature, and concentrations of reactants and products.

The equilibrium constant for a reaction, which can be calculated using the Nernst equation and the standard cell potential.

The condition where the chemical potential of all reactants and products in a reaction are equal, leading to no net change in concentration.

The reaction quotient, which is similar to the equilibrium constant, but it measures the relative amounts of reactants and products at any point during a reaction.

A measure of the spontaneity or feasibility of a reaction. A positive value indicates a spontaneous reaction, while a negative value indicates a non-spontaneous reaction.

The potential difference between two half-cells when the cell is at equilibrium. It is zero for any reversible cell at equilibrium.

A measure of the acidity or alkalinity of a solution. It is defined as the negative logarithm of the hydrogen ion concentration.

A process that involves the movement of charged particles through a conductor due to a difference in electrical potential. It is the flow of electrical charge.

The ability of a substance to conduct electricity. It depends on the concentration of charge carriers and their mobility.

A chemical reaction that involves the transfer of electrons between reactants.

A substance that loses electrons in a redox reaction, causing the oxidation of another substance.

A substance that gains electrons in a redox reaction, causing the reduction of another substance.

The tendency of a species to gain electrons and undergo reduction. It is measured in volts and can be used to predict the feasibility of redox reactions.