Textbook Question
What is the pH of the solution in the cathode compartment of the following cell if the measured cell potential at 25 °C is 0.17 V?
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Ch.19 - Electrochemistry
Chapter 19, Problem 112
Calculate the equilibrium constant at 25 °C for the reaction
Verified step by step guidance1
Step 1: Identify the balanced chemical equation for the reaction. This will help you determine the stoichiometry of the reactants and products involved.
Step 2: Write the expression for the equilibrium constant, K, using the balanced chemical equation. The general form is K = [products]^coefficients / [reactants]^coefficients, where the concentrations are at equilibrium.
Step 3: Determine the standard Gibbs free energy change (ΔG°) for the reaction at 25 °C. This can be done using tabulated standard Gibbs free energies of formation for the reactants and products.
Step 4: Use the relationship between the equilibrium constant and the Gibbs free energy change: ΔG° = -RT ln(K), where R is the universal gas constant (8.314 J/mol·K) and T is the temperature in Kelvin (298 K for 25 °C).
Step 5: Rearrange the equation from Step 4 to solve for the equilibrium constant, K, by calculating K = e^(-ΔG°/RT).
Related Practice
Textbook Question
Beginning with the equations that relate E°, ∆G°, and K, show that ∆G° is negative and K 7 1 for a reaction that has a positive value of E°
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Textbook Question
If a reaction has an equilibrium constant K 6 1, is E° posi-tive or negative? What is the value of K when E° = 0 V?
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Open Question
Calculate the equilibrium constant at 25 °C for the reaction
Open Question
Calculate the equilibrium constant at 25 °C for the reaction . See Appendix D for standard reduction potentials.
Textbook Question
The following galvanic cell has a potential of 1.214 V at 25 °C: Calculate the value of Ksp for Hg2Br2 at 25°C
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