If 4.00 g of metal is plated in the voltaic cell (which contains Ag and Ni with the total potential of 2.98 V) , how much metal is plated in the electrolytic cell (contains Ag and Zn with the total of 1.98 V)?
I have no idea how to do this! Help?
To solve this problem, you need to understand the relationship between the amount of metal plated in a voltaic cell and an electrolytic cell.
In a voltaic cell, the transfer of electrons occurs spontaneously due to the potential difference between the two electrodes. The metal with the highest reduction potential is plated out as it gains electrons.
On the other hand, in an electrolytic cell, an external power source (e.g., a battery) is used to force the transfer of electrons. The metal with the lowest reduction potential is plated out as it gains electrons.
To solve the problem, we need to compare the reduction potentials of the metals in each cell and understand their behavior.
1. Determine the metal that gets plated in the voltaic cell:
- Calculate the standard reduction potential for each metal (Ag and Ni) relative to the standard hydrogen electrode (SHE). Consult a table of standard reduction potentials.
- Determine which metal has the higher reduction potential. The metal with the higher reduction potential will be plated out in the voltaic cell.
2. Determine the metal that gets plated in the electrolytic cell:
- Calculate the reduction potential for each metal (Ag and Zn) relative to the standard hydrogen electrode (SHE). The reduction potential is the potential difference between the two electrodes in the electrolytic cell.
- Determine which metal has the lower reduction potential. The metal with the lower reduction potential will be plated out in the electrolytic cell.
3. Calculate the amount of metal plated in the electrolytic cell:
- Use the Faraday's law of electrolysis, which states that the amount of metal plated is directly proportional to the amount of charge passed through the cell.
- The charge, Q, can be calculated using the formula: Q = I * t, where I is the current passing through the cell and t is the time.
- The amount of metal plated can be calculated using the formula: n = Q / F, where n is the moles of metal plated and F is Faraday's constant (96485 C/mol). We can assume the molar mass of the metal is known to convert this into grams.
By following these steps, you should be able to determine the amount of metal plated in the electrolytic cell. Remember to consult standard reduction potentials and use the appropriate formulas for your calculations.