객관식
At 25°C, E° = +1.88 V for a cell based on the reaction 3 AgCl(s) + Al(s) → 3 Ag(s) + Al³⁺(aq) + 3 Cl⁻(aq). Find the cell potential E if [Al³⁺] = 0.20 M and [Cl⁻] = 0.010 M using the Nernst equation.
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20. Electrochemistry
Cell Potential: The Nernst Equation
객관식
What is the change in the cell voltage when the ion concentrations in the cathode half-cell are increased by a factor of 10, according to the Nernst Equation?
A
The cell voltage increases by 0.059 V
B
The cell voltage decreases by 0.059 V
C
The cell voltage decreases by 0.1 V
D
The cell voltage remains unchanged
검증된 단계별 안내1
Identify the Nernst Equation: The Nernst Equation is used to calculate the cell potential under non-standard conditions. It is given by: , where is the cell potential, is the standard cell potential, and is the number of moles of electrons transferred in the reaction.
Determine the effect of increasing ion concentration: Increasing the concentration of ions in the cathode half-cell by a factor of 10 affects the reaction quotient in the Nernst Equation. Specifically, the concentration of products in the reaction quotient increases.
Calculate the change in the reaction quotient: Since the concentration of ions in the cathode half-cell is increased by a factor of 10, the reaction quotient becomes 10 times larger.
Apply the change to the Nernst Equation: Substitute the new value of into the Nernst Equation. The logarithmic term will increase by , which is 1.
Determine the change in cell voltage: The increase in the logarithmic term by 1 results in a decrease in the cell voltage by volts. Since is typically 1 for a single electron transfer, the cell voltage decreases by 0.059 V.
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