Physics Formulas
NEET Biology Physics Chemistry question and answer by careeradvice.in
@careeradvice_in
The best NEET guidance, NEET tips and tricks, Get free NEET mocks, Neet updates. All news and updates related to NEET at one place.
#neet2023
NEET Biology Physics Chemistry question and answer by careeradvice.in (English)
Are you a NEET aspirant looking for the best guidance and tips to excel in your exams? Look no further! Welcome to the official Telegram channel of careeradvice.in, where you can find all the resources you need to succeed in NEET. From biology to physics to chemistry, we have got you covered with expertly crafted questions and answers that will help you ace your exams.
Our channel is dedicated to providing NEET aspirants with valuable tips and tricks that will enhance their preparation. Whether you are aiming for NEET 2023 or planning ahead for future exams, our channel is the perfect place to stay updated with the latest news and updates related to NEET.
By joining our channel, you will have access to free NEET mocks that will help you assess your strengths and weaknesses. Our team of experienced educators is committed to providing you with the tools you need to succeed in your NEET journey.
Don't miss out on this opportunity to receive comprehensive guidance on NEET preparation. Join careeradvice.in's Telegram channel today and take the first step towards achieving your dream of becoming a successful medical professional. #neet2023
NEET Biology Physics Chemistry question and answer by careeradvice.in
05 Dec, 05:32
Liquid Solution Short Notes
NEET Biology Physics Chemistry question and answer by careeradvice.in
03 Dec, 05:32
Nitrogen Family Handwritten Notes
NEET Biology Physics Chemistry question and answer by careeradvice.in
02 Dec, 05:32
Important Notes - Electrochemical Cells
► An electrochemical cell can convert electrical energy to chemical energy and can also convert electrical energy to chemical energy. There are two types of electrochemical cells- Galvanic cell and Electrolytic cell.
► Cathodes are usually metal electrodes. It is the electrode where reduction takes place. The cathode is the positive electrode in a galvanic cell and a negative electrode in an electrolytic cell. Electrons move into the cathode.
► A half-cell is half of an electrochemical cell (electrolytic or galvanic), where either oxidation or reduction occurs. At equilibrium, there is no transfer of electrons across the half cells. Therefore, the potential difference between them is nil.
► A salt bridge is a device used to connect the oxidation and reduction half-cells of a galvanic cell (a type of electrochemical cell). Strong electrolytes are generally used to make the salt bridges in electrochemical cells. Since ZnSO4 is not a strong electrolyte, it is not used to make salt bridges.
► Emf of a cell is equal to the maximum potential difference across its electrodes, which occurs when no current is drawn through the cell. It can also be defined as the net voltage between the oxidation and reduction half-reactions.
► Cell potential is an intensive property as it is independent of the amount of material present. Gibbs free energy is defined for an electrochemical cell and is an extensive property as it depends on the quantity of the material.
► Electrode potential is the tendency of an electrode to accept or to lose electrons. Electrode potential depends on the nature of the electrode, temperature of the solution and the concentration of metal ions in the solution. It doesn’t depend on the size of the electrode.
► The salt bridge connects the two half-cell solutions to complete the circuit of the electrochemical cell. The electrolytes of the salt bridge are generally prepared in agar-agar or gelatin so that the electrolytes are kept in a semi-solid phase and do not mix with the half-cell solutions and interfere with the electrochemical reaction.
► A salt bridge is a junction that connects the anodic and cathodic compartments in a cell or electrolytic solution. It maintains electrical neutrality within the internal circuit, preventing the cell from rapidly running its reaction to equilibrium.
► A Voltaic or Galvanic cell is a type of electrochemical cell that converts chemical energy into electrical energy. Photovoltaic cells are used to convert light energy into electrical energy. An Electrolytic cell is a type of electrochemical cell that converts electrical energy into chemical energy. A fuel cell is an electrochemical cell that converts the chemical energy of a fuel and an oxidizing agent into electricity.
► For all spontaneous chemical reactions, the change in Gibbs free energy (ΔG°) is always negative. For a spontaneous reaction in an electrolytic cell, the cell potential (E°cell) should be positive.
► In an electrochemical cell, when an opposing externally potential is applied and increased slowly, the reaction continues to take place. When the external potential is equal to the potential of the cell, the reaction stops. Once the externally applied potential is greater than the potential of the cell, the reaction goes in the opposite direction and the cell behaves like an electrolytic cell.
► Primary cells cannot be used again and again. Since there is no fluid inside, these cells are also known as dry cells. The internal resistance is high and the chemical reaction is irreversible. Their initial cost is cheap.
► A secondary battery (a series of cells) is one which can be charged, discharged into a load, and recharged many times. Nickel-cadmium cell, Lead storage cell and Mercury cell are examples of secondary cells. Leclanche cell is an example of a primary cell.
► An electrochemical cell can convert electrical energy to chemical energy and can also convert electrical energy to chemical energy. There are two types of electrochemical cells- Galvanic cell and Electrolytic cell.
► Cathodes are usually metal electrodes. It is the electrode where reduction takes place. The cathode is the positive electrode in a galvanic cell and a negative electrode in an electrolytic cell. Electrons move into the cathode.
► A half-cell is half of an electrochemical cell (electrolytic or galvanic), where either oxidation or reduction occurs. At equilibrium, there is no transfer of electrons across the half cells. Therefore, the potential difference between them is nil.
► A salt bridge is a device used to connect the oxidation and reduction half-cells of a galvanic cell (a type of electrochemical cell). Strong electrolytes are generally used to make the salt bridges in electrochemical cells. Since ZnSO4 is not a strong electrolyte, it is not used to make salt bridges.
► Emf of a cell is equal to the maximum potential difference across its electrodes, which occurs when no current is drawn through the cell. It can also be defined as the net voltage between the oxidation and reduction half-reactions.
► Cell potential is an intensive property as it is independent of the amount of material present. Gibbs free energy is defined for an electrochemical cell and is an extensive property as it depends on the quantity of the material.
► Electrode potential is the tendency of an electrode to accept or to lose electrons. Electrode potential depends on the nature of the electrode, temperature of the solution and the concentration of metal ions in the solution. It doesn’t depend on the size of the electrode.
► The salt bridge connects the two half-cell solutions to complete the circuit of the electrochemical cell. The electrolytes of the salt bridge are generally prepared in agar-agar or gelatin so that the electrolytes are kept in a semi-solid phase and do not mix with the half-cell solutions and interfere with the electrochemical reaction.
► A salt bridge is a junction that connects the anodic and cathodic compartments in a cell or electrolytic solution. It maintains electrical neutrality within the internal circuit, preventing the cell from rapidly running its reaction to equilibrium.
► A Voltaic or Galvanic cell is a type of electrochemical cell that converts chemical energy into electrical energy. Photovoltaic cells are used to convert light energy into electrical energy. An Electrolytic cell is a type of electrochemical cell that converts electrical energy into chemical energy. A fuel cell is an electrochemical cell that converts the chemical energy of a fuel and an oxidizing agent into electricity.
► For all spontaneous chemical reactions, the change in Gibbs free energy (ΔG°) is always negative. For a spontaneous reaction in an electrolytic cell, the cell potential (E°cell) should be positive.
► In an electrochemical cell, when an opposing externally potential is applied and increased slowly, the reaction continues to take place. When the external potential is equal to the potential of the cell, the reaction stops. Once the externally applied potential is greater than the potential of the cell, the reaction goes in the opposite direction and the cell behaves like an electrolytic cell.
► Primary cells cannot be used again and again. Since there is no fluid inside, these cells are also known as dry cells. The internal resistance is high and the chemical reaction is irreversible. Their initial cost is cheap.
► A secondary battery (a series of cells) is one which can be charged, discharged into a load, and recharged many times. Nickel-cadmium cell, Lead storage cell and Mercury cell are examples of secondary cells. Leclanche cell is an example of a primary cell.
NEET Biology Physics Chemistry question and answer by careeradvice.in
30 Nov, 05:32
Hydrocarbon Short Notes
NEET Biology Physics Chemistry question and answer by careeradvice.in
28 Nov, 05:33
Rotational Motion & Fluids
Short Notes
Short Notes
NEET Biology Physics Chemistry question and answer by careeradvice.in
27 Nov, 05:33
Examples of Common Names and IUPAC of important Organic Compounds
NEET Biology Physics Chemistry question and answer by careeradvice.in
26 Nov, 05:32
Hydrogen Derivatives Notes
NEET Biology Physics Chemistry question and answer by careeradvice.in
25 Nov, 05:32
Chemical Bonding Short Notes
NEET Biology Physics Chemistry question and answer by careeradvice.in
24 Nov, 05:32
Atomic Structure
NEET Biology Physics Chemistry question and answer by careeradvice.in
21 Nov, 05:32
Magnetism Short Notes
NEET Biology Physics Chemistry question and answer by careeradvice.in
20 Nov, 05:33
KTG & Thermodynamics
Short Notes
Short Notes
NEET Biology Physics Chemistry question and answer by careeradvice.in
19 Nov, 05:33
Current Electricity Short Notes
NEET Biology Physics Chemistry question and answer by careeradvice.in
21 Oct, 06:57
𝐏𝐇𝐘𝐒𝐈𝐂𝐀𝐋 𝐏𝐑𝐎𝐏𝐄𝐑𝐓𝐈𝐄𝐒 𝐎𝐅 𝐏𝐇𝐄𝐍𝐎𝐋𝐒
▸ Phenols are colorless crystalline solid or liquid having a characteristic odour.
▸ Due to hydrogen bonding phenols has higher boiling point.
▸ The solubility of phenols in water is decreases with increase in size of aryl groups. Hydrophobic character increases as number of aryl groups increases
▸ Phenols are colorless crystalline solid or liquid having a characteristic odour.
▸ Due to hydrogen bonding phenols has higher boiling point.
▸ The solubility of phenols in water is decreases with increase in size of aryl groups. Hydrophobic character increases as number of aryl groups increases
3,706
subscribers
485
photos
1
videos
