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A concentration cell is a type of electrochemical cell where both the cathode and anode are made of the same material, while the electrolyte solutions have different concentrations. The voltage generated by a concentration cell is due to the difference in concentrations of the same species in each half-cell. The overall cell potential of a concentration cell is a result of the concentration gradient of the half cells, which drives the movement of the ions and creates a charge flow.

The standard reduction potential (E°) is a measurement of the inherent voltage (or tendency) of a half-cell reaction to occur under standard conditions (i.e., temperature, pressure, and concentration). The value of the standard reduction potential is determined with respect to the hydrogen electrode, which has a potential of 0 V by definition.

Standard reduction potentials (E°) are defined under standard conditions, and they are constants for a given half-cell reaction. However, the actual cell potential (E) may vary depending on the concentrations of the reacting species. This relationship is governed by the Nernst equation: \[E = E° - \frac{RT}{nF} \ln Q\] Where: - E is the actual cell potential - E° is the standard cell potential - R is the gas constant - T is the absolute temperature - n is the number of moles of electrons exchanged in the redox reaction - F is the Faraday constant - Q is the reaction quotient, which represents the ratios of the concentrations of reactants and products From the Nernst equation, we can see that the actual cell potential (E) is affected by the concentration of reactants and products. However, the standard reduction potential (E°) remains constant.

The statement "Concentration cells work because standard reduction potentials are dependent on concentration" is false. Although the actual cell potential (E) is influenced by the concentration of reactants and products, the standard reduction potential (E°) remains constant. In concentration cells, the voltage generated is due to the concentration gradient of the half-cells and not because of a change in the standard reduction potentials.