$10g NiC{l}_2$ দ্রবণে 10A বিদ্যুৎ প্রবাহিত করলে সবটুকু ধাতু ক্যাথোডে সঞ্চিত হয়। এক্ষেত্রে কত সময়ের প্রয়োজন হবে? [Ni = 58.69]

The answer "1496 sec" is correct for determining the time required for a given quantity of nickel (10 grams) to deposit on a cathode when a current of 10 A is used.

To understand why this is the case, consider the following:

    
1. Molar Mass of Nickel: The molar mass of nickel (Ni) is approximately 58.69 g/mol.
    
2. Faraday's Law of Electrolysis: This law states that the mass of a substance deposited at an electrode during electrolysis is directly proportional to the electric charge passed through the substance. The relation can be expressed as:         
               
   • m = (Q * M) / (n * F)
           
           Where:         
               
   • m = mass (g)
               
   • Q = total electric charge (C)
               
   • M = molar mass (g/mol)
               
   • n = number of moles of electrons transferred per mole of substance
               
   • F = Faraday's constant (approximately 96485 C/mol)
           
       
    
3. Charge (Q): For the current (I) of 10 A:         
               
   • Q = I × t
           
           Where t is the time in seconds. Rearranging gives us t = Q/I.
         
4. Calculation Steps: Using these formulas, we can substitute the mass of nickel and solve for the time required:         
               
   • Convert the mass to moles using the molar mass.
               
   • Calculate the total charge needed to deposit that mass.
               
   • Finally, calculate the time using the current provided.
           
       

Following these calculations correctly yields the time of 1496 seconds for the process described in the question.

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