Class 12 Exam > Class 12 Videos > Daniel Cell - Electrochemistry, Class 12
Daniel Cell - Electrochemistry, Class 12 Video Lecture
FAQs on Daniel Cell - Electrochemistry, Class 12 Video Lecture
| 1. What is electrochemistry? |  |
Ans. Electrochemistry is a branch of chemistry that deals with the study of the relationship between electricity and chemical reactions. It involves the conversion of chemical energy into electrical energy or vice versa. This field focuses on the movement of electrons during chemical reactions.
| 2. What are the applications of electrochemistry? | |
Ans. Electrochemistry finds various applications in different fields. Some of the significant applications include:
1. Batteries and fuel cells: Electrochemistry plays a crucial role in the functioning of batteries and fuel cells, which are used to store and produce electrical energy, respectively.
2. Corrosion prevention: Electrochemical techniques are used to prevent or reduce the corrosion of metals by applying protective coatings or sacrificial anodes.
3. Electroplating: It is a process in which a metal object is coated with a thin layer of another metal using electrolysis. This technique is commonly used in industries for decorative purposes or to enhance the durability of objects.
4. Sensors: Electrochemical sensors are widely used to detect and measure the concentration of various substances in fields like environmental monitoring, healthcare, and food safety.
5. Electrolysis: Electrolysis is the process of using an electric current to drive a non-spontaneous chemical reaction. It is applied in industries for the production of metals like aluminum, copper, and chlorine gas.
| 3. What is the role of electrodes in electrochemistry? | |
Ans. Electrodes play a crucial role in electrochemistry as they provide the surface where the desired chemical reactions take place. There are two types of electrodes: anode and cathode.
The anode is the electrode where oxidation (loss of electrons) occurs, while the cathode is the electrode where reduction (gain of electrons) takes place. These reactions are necessary for the flow of current and the generation of electricity in electrochemical cells.
The choice of material for electrodes is essential as it can influence the reaction rates and overall efficiency of the electrochemical process. Common electrode materials include platinum, graphite, and various metal alloys.
| 4. What is the Nernst equation? | |
Ans. The Nernst equation is an equation that relates the standard electrode potential, temperature, and concentration of species involved in an electrochemical reaction. It is used to determine the cell potential under non-standard conditions.
The Nernst equation is given by:
E = E° - (0.0592/n) * log(Q)
Where:
- E is the cell potential under non-standard conditions
- E° is the standard electrode potential
- n is the number of electrons involved in the reaction
- Q is the reaction quotient, which is the ratio of product concentrations to reactant concentrations
The Nernst equation allows for the calculation of the cell potential at any given concentration and temperature, providing a more accurate representation of the electrochemical system.
| 5. What is Faraday's law of electrolysis? | |
Ans. Faraday's law of electrolysis states that the amount of chemical reaction at an electrode during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte.
Mathematically, it can be expressed as:
m = (Z * I * t) / F
Where:
- m is the mass of the substance undergoing a chemical reaction
- Z is the electrochemical equivalent, which is the amount of substance deposited or produced per unit charge
- I is the current passing through the electrolyte
- t is the time for which the current is passed
- F is Faraday's constant, which represents the charge of one mole of electrons
Faraday's law allows for the calculation of the amount of substance produced or consumed during an electrolysis process, providing a quantitative understanding of electrochemical reactions.
Text Transcript from Video
here is a setup for Daniel cell it
contains two containers one has a copper
sulphate solution and the other has zinc
sulfate solution let us now take a zinc
rod and dip it in zinc sulphate solution
and let's dip a copper rod in copper
sulfate solution now let's connect the
two rods using wires and we also put a
switch and a voltmeter the two solutions
are also connected using a salt bridge
which has an inert electrolyte for
example potassium nitrate now as soon as
the switch is closed to complete the
circuit current starts flowing from
copper electrode to the zinc electrode
and that can be confirmed by the
deflection of needle in the voltmeter
let me write down the reaction that
takes place at the zinc electrode so as
you can see zinc gets oxidized and acts
as anode now two electrons are released
in the process these two electrons are
then transferred by the wires to the
copper electrode where they are absorbed
by the Cu 2 plus ions to form copper so
copper electrode acts as a cathode and
here is the reaction that takes place at
the cathode so what is the net reaction
that takes place in Danial cell here it
is
contains two containers one has a copper
sulphate solution and the other has zinc
sulfate solution let us now take a zinc
rod and dip it in zinc sulphate solution
and let's dip a copper rod in copper
sulfate solution now let's connect the
two rods using wires and we also put a
switch and a voltmeter the two solutions
are also connected using a salt bridge
which has an inert electrolyte for
example potassium nitrate now as soon as
the switch is closed to complete the
circuit current starts flowing from
copper electrode to the zinc electrode
and that can be confirmed by the
deflection of needle in the voltmeter
let me write down the reaction that
takes place at the zinc electrode so as
you can see zinc gets oxidized and acts
as anode now two electrons are released
in the process these two electrons are
then transferred by the wires to the
copper electrode where they are absorbed
by the Cu 2 plus ions to form copper so
copper electrode acts as a cathode and
here is the reaction that takes place at
the cathode so what is the net reaction
that takes place in Danial cell here it
is
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Oct 26, 2024 Last updated |
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