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In a Daniel cell,...

In a Daniel cell,

A

the chemical energy liberted during the redox reaction is converted to electrical energy

B

the electrical energy of the cell is converted to chemical energy

C

the energy of the cell is utilised in conduction of the redox reaction

D

the potential energy of the cell is converted into electrical energy.

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question regarding the Daniel cell, we will analyze the components and reactions occurring in the cell step by step. ### Step 1: Understanding the Daniel Cell A Daniel cell is a type of galvanic cell that converts chemical energy into electrical energy through redox reactions. It consists of two half-cells: one containing zinc and the other containing copper. **Hint:** Remember that a galvanic cell generates electricity from spontaneous chemical reactions. ### Step 2: Identifying the Anode and Cathode In a Daniel cell: - The anode is where oxidation occurs. In this case, zinc (Zn) is oxidized to zinc ions (Zn²⁺). - The cathode is where reduction occurs. Copper ions (Cu²⁺) are reduced to solid copper (Cu). **Hint:** Oxidation involves the loss of electrons, while reduction involves the gain of electrons. ### Step 3: Writing the Half-Reactions At the anode: \[ \text{Zn} \rightarrow \text{Zn}^{2+} + 2e^- \] At the cathode: \[ \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu} \] **Hint:** Each half-reaction shows the process occurring at the respective electrodes. ### Step 4: Overall Cell Reaction Combining the half-reactions, we get the overall reaction for the Daniel cell: \[ \text{Zn} + \text{Cu}^{2+} \rightarrow \text{Zn}^{2+} + \text{Cu} \] **Hint:** The overall reaction represents the transfer of electrons from the anode to the cathode. ### Step 5: Energy Conversion In a Daniel cell, the chemical energy released during the redox reaction is converted into electrical energy. This is the fundamental principle behind the operation of galvanic cells. **Hint:** Focus on the relationship between chemical reactions and energy conversion. ### Conclusion Thus, the correct statement regarding the Daniel cell is that it is a galvanic cell where zinc acts as the anode and copper as the cathode, and the chemical energy liberated during the redox reaction is converted into electrical energy. ### Final Answer: - The correct option is that the chemical energy liberated during the redox reaction is converted into electrical energy.
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The most pupular electrochemical cell, daniel cell was originally developed by the English chemist john F daniel the general assembly of the cell is as given below An undergraduate student made a Daniel cell using 100cm^(3) of 0.100MCuSO_(4) ad 0.100M ZnSO_(4) solution respectively. The two compartments are connected by suitable salt bridge. [given E_((Cu^(2+)//Cu))^(@)=0.34V,E_((Zn^(2+)//Zn))=-0.76V,(2.30RT)/(F)=0.06,log2=0.3] Q. Calculate the emf (in volt) of the above cell.

The most pupular electrochemical cell, daniel cell was originally developed by the English chemist john F daniel the general assembly of the cell is as given below An undergraduate student made a Daniel cell using 100cm^(3) of 0.100MCuSO_(4) ad 0.100M ZnSO_(4) solution respectively. The two compartments are connected by suitable salt bridge. [given E_((Cu^(2+)//Cu))^(@)=0.34V,E_((Zn^(2+)//Zn))=-0.76V,(2.30RT)/(F)=0.06,log2=0.3] Q. A labmate of the student asked her for some solid CuCl_(2) . while she was lifting the bottle from a shelf, the lid of the bottle slipped and some amount of CuCl_(2) fell in the CuSO_(4) compartment at constant volume. She measured the emf of the cell again and found that it has increase by 9 mV. She used this data to calculate the amount of CuCl_(2) that had spilled in the compartment. Calculate the mass of CuCl_(2) that had spilled into the daniel cell? (molar mass of CuCl_(2)=135(g)/(mol))

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