EC PPT CIVIL, daniel cell, woring of daniel cell

daniel cell, woring of daniel cell

1. ENGINEERING CHEMISTRY   Submitted by: 241FA03003 – Rishitha 241FA03005 – Jashuva 241FA03013 – karthik 241FA03016 -   Akhil Submitted to: Faculty Name : Dr . N. Satya Vijaya Kumar CIVIL ENGINEERING BATCH-03      

2. DANIEL CELL: The Daniel cell is a type of electrochemical cell invented by British chemist John Frederic Daniel in 1836. It is a copper pot and copper sulphate battery that produces a steady electric current . Key Components : 1.Copper Pot: The copper pot serves as the anode (negative electrode) of the cell . 2.Copper Sulphate Solution: The copper sulphate solution is the electrolyte that facilitates the flow of electric current. 3.Copper Sulphate Crystals: The copper sulphate crystals are used to maintain the concentration of the electrolyte.

3. WORKING OF DANIEL CELL : Step 1: Oxidation at the Anode- The Daniel cell consists of a copper pot (anode) and a zinc rod (cathode) immersed in a copper sulphate solution.- At the anode, copper is oxidized to form copper ions (Cu²⁺), releasing electrons . Step 2: Reduction at the Cathode- At the cathode, zinc is reduced to form zinc metal, absorbing electrons.- The zinc metal is deposited on the surface of the zinc rod . Step 3: Ion Flow through the Salt Bridge- The copper sulphate solution is connected to a salt bridge, which is a tube filled with a potassium nitrate solution.- The salt bridge allows ions to flow between the two solutions, maintaining electrical neutrality . Step 4: Electron Flow through the External Circuit- The electrons released at the anode flow through the external circuit to the cathode.- The external circuit can be a wire, a resistor, or any other device that allows electrons to flow . Step 5: Chemical Reaction at the Anode and Cathode- At the anode, the copper ions (Cu²⁺) react with the sulphate ions (SO₄²⁻) to form copper sulphate (CuSO₄).- At the cathode, the zinc metal (Zn) reacts with the sulfate ions (SO₄²⁻) to form zinc sulfate (ZnSO₄ ). Step 6: Cell Discharge- As the cell operates, the copper anode is gradually consumed, and the zinc cathode is gradually deposited.- The cell continues to operate until the copper anode is completely consumed or the zinc cathode is fully deposited.

4. HALF CELL REACTIONS: .

5. EMF OF THE CONSTRUCTED CELL AT STP CONDITIONS : ​ . Oxidation (anode): Zn(s) Zn2+(aq) + 2 Reduction (cathode): Cu²+(aq) + 2e-Cu(s) The standard reduction potentials are: E_Zn2+/Zn = -0.76 V E°_Cu²+/Cu = +0.34 V The number of electrons transferred is 2. Calculation: E_cell = E°_cathode - E"_anode =E_Cu2+/Cu - E_Zn2+/Zn (+0.34 V)-(-0.76 V) = +1.10 V Therefore, the EMF of the constructed cell at STP conditions is +1.10 V.

6. ELUCIDATE THE USE AND IMPOTACE OF SALT BRIDGE : A salt bridge is a crucial component in a Daniel cell, and it plays a vital role in the functioning of the cell . Use of Salt Bridge: A salt bridge is used to connect the two half-cells of a Daniel cell, allowing ions to flow between them while keeping the electrodes separate. Importance of Salt Bridge : 1.Maintains Electrical Neutrality: The salt bridge helps maintain electrical neutrality in the cell by allowing ions to flow between the half-cells, balancing the charges . 2. Prevents Electrode Polarization: The salt bridge prevents electrode polarization by allowing ions to flow and maintain the electrode's potential . 3 . Enables Ion Flow: The salt bridge enables the flow of ions between the half-cells, which is necessary for the cell reaction to occur . 4 . Stabilizes Cell Potential: The salt bridge helps stabilize the cell potential by maintaining a consistent ion flow and preventing large changes in the electrode potentials.