An electrochemical cell consists of a standard hydrogen...

An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a. What is the potential of the cell at $25^{\circ} \mathrm{C}$ if the copper electrode is placed in a solution in which $\left[\mathrm{Cu}^{2+}\right]=2.5 \times 10^{-4} M ?$ b. The copper electrode is placed in a solution of unknown $\left[\mathrm{Cu}^{2+}\right]$. The measured potential at $25^{\circ} \mathrm{C}$ is $0.195 \mathrm{~V}$. What is $\left[\mathrm{Cu}^{2+}\right] ?$ (Assume $\mathrm{Cu}^{2+}$ is reduced.)

An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode.
a. What is the potential of the cell at $25^{\circ} \mathrm{C}$ if the copper electrode is placed in a solution in which $\left[\mathrm{Cu}^{2+}\right]=2.5 \times 10^{-4} M ?$
b. The copper electrode is placed in a solution of unknown $\left[\mathrm{Cu}^{2+}\right]$. The measured potential at $25^{\circ} \mathrm{C}$ is $0.195 \mathrm{~V}$. What is $\left[\mathrm{Cu}^{2+}\right] ?$ (Assume $\mathrm{Cu}^{2+}$ is reduced.)

Key Concepts

Electrochemical Cell

An electrochemical cell is a device that converts chemical energy into electrical energy (or vice versa) via redox reactions. It consists of two half-cells, each containing an electrode and an electrolyte, connected by a conductive pathway that allows electron transfer and often a salt bridge to maintain ion balance.

Standard Hydrogen Electrode (SHE)

The Standard Hydrogen Electrode is a reference electrode with a defined potential of 0.00 V under standard conditions by convention. It is used as the baseline for measuring and comparing the electrode potentials of other half-cells in polarography and electrochemistry.

Reduction and Oxidation Reactions

Redox reactions involve the transfer of electrons between chemical species. In an electrochemical cell, one electrode undergoes oxidation (loss of electrons) while the other undergoes reduction (gain of electrons). Understanding which species is reduced or oxidized is essential for determining the cell's overall potential.

Standard Reduction Potential

Standard reduction potentials are intrinsic values that measure the tendency of a chemical species to be reduced under standard conditions. They serve as benchmarks to predict the direction of redox reactions, and the difference between the potentials of two half-cells determines the overall cell voltage.

Nernst Equation

The Nernst equation provides a relationship between the electrode potential and the activities (or concentrations) of the reactants and products involved in the redox process. It allows the calculation of the electrode potential under non-standard conditions by accounting for the effects of concentration and temperature on the cell potential.

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