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For the half-cell,at 298K electrode potential has maximum value when KCl used is a)1 M b)0.1 M c)0.01 M d)10 M Correct answer is option 'C'. Can you explain this answer?
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For the half-cell,at 298K electrode potential has maximum value when K...
Explanation:
In order to understand why the electrode potential has a maximum value when the concentration of KCl is 0.01 M, we need to consider the Nernst equation and the concept of activity.
The Nernst equation relates the electrode potential (E) to the concentrations (or activities) of the species involved in the half-cell reaction. It is given by:
E = E° - (RT/nF) * ln(Q)
Where:
- E is the electrode potential
- E° is the standard electrode potential
- R is the gas constant (8.314 J/(mol·K))
- T is the temperature in Kelvin
- n is the number of electrons transferred in the half-cell reaction
- F is the Faraday constant (96500 C/mol)
- Q is the reaction quotient, which is the ratio of product concentrations to reactant concentrations raised to their stoichiometric coefficients.
Effect of Concentration:
The concentration of KCl affects the reaction quotient (Q) in the Nernst equation. As the concentration of KCl increases, the concentration of K+ ions also increases, which affects the activity of K+. The activity of an ion is a measure of its effective concentration, taking into account factors such as ionic strength and ion-ion interactions.
Effect on Electrode Potential:
When the concentration of KCl is very low (0.01 M), the activity of K+ ions is close to their concentration. As a result, the reaction quotient (Q) in the Nernst equation is closer to 1, and the logarithmic term in the equation becomes small. This leads to a higher electrode potential.
On the other hand, when the concentration of KCl is very high (1 M), the activity of K+ ions significantly deviates from the concentration due to increased ionic interactions and ionic strength. This results in a larger value for the logarithmic term in the Nernst equation, leading to a lower electrode potential.
Therefore, the electrode potential has a maximum value when the concentration of KCl is 0.01 M, as this concentration provides the optimal conditions for the activity of K+ ions and minimizes deviations from the concentration.
Conclusion:
In summary, the electrode potential has a maximum value when the concentration of KCl used is 0.01 M. This is because at this concentration, the activity of K+ ions is close to their concentration, leading to a smaller logarithmic term in the Nernst equation and a higher electrode potential.
In order to understand why the electrode potential has a maximum value when the concentration of KCl is 0.01 M, we need to consider the Nernst equation and the concept of activity.
The Nernst equation relates the electrode potential (E) to the concentrations (or activities) of the species involved in the half-cell reaction. It is given by:
E = E° - (RT/nF) * ln(Q)
Where:
- E is the electrode potential
- E° is the standard electrode potential
- R is the gas constant (8.314 J/(mol·K))
- T is the temperature in Kelvin
- n is the number of electrons transferred in the half-cell reaction
- F is the Faraday constant (96500 C/mol)
- Q is the reaction quotient, which is the ratio of product concentrations to reactant concentrations raised to their stoichiometric coefficients.
Effect of Concentration:
The concentration of KCl affects the reaction quotient (Q) in the Nernst equation. As the concentration of KCl increases, the concentration of K+ ions also increases, which affects the activity of K+. The activity of an ion is a measure of its effective concentration, taking into account factors such as ionic strength and ion-ion interactions.
Effect on Electrode Potential:
When the concentration of KCl is very low (0.01 M), the activity of K+ ions is close to their concentration. As a result, the reaction quotient (Q) in the Nernst equation is closer to 1, and the logarithmic term in the equation becomes small. This leads to a higher electrode potential.
On the other hand, when the concentration of KCl is very high (1 M), the activity of K+ ions significantly deviates from the concentration due to increased ionic interactions and ionic strength. This results in a larger value for the logarithmic term in the Nernst equation, leading to a lower electrode potential.
Therefore, the electrode potential has a maximum value when the concentration of KCl is 0.01 M, as this concentration provides the optimal conditions for the activity of K+ ions and minimizes deviations from the concentration.
Conclusion:
In summary, the electrode potential has a maximum value when the concentration of KCl used is 0.01 M. This is because at this concentration, the activity of K+ ions is close to their concentration, leading to a smaller logarithmic term in the Nernst equation and a higher electrode potential.
Community Answer
For the half-cell,at 298K electrode potential has maximum value when K...
C is correct bro
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For the half-cell,at 298K electrode potential has maximum value when KCl used is a)1 M b)0.1 M c)0.01 M d)10 M Correct answer is option 'C'. Can you explain this answer?
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