Textbook Question
Use tabulated electrode potentials to calculate ∆G°rxn for each reaction at 25 °C. b. Br2(l) + 2 Cl–(aq) → 2 Br–(aq) + Cl2(g) c. MnO2(s) + 4 H+(aq) + Cu(s) → Mn2+(aq) + 2 H2O(l) + Cu2+(aq)
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Ch.19 - Electrochemistry
Chapter 19, Problem 68
What is the equilibrium constant for each of the reactions mentioned in Problem 66?
Verified step by step guidance1
insert step 1> Identify the reactions mentioned in Problem 66.
insert step 2> Write the balanced chemical equation for each reaction.
insert step 3> Use the balanced equations to write the expression for the equilibrium constant (K) for each reaction.
insert step 4> Determine the concentrations or partial pressures of the reactants and products at equilibrium, if provided.
insert step 5> Substitute the equilibrium concentrations or partial pressures into the equilibrium constant expression to solve for K.
Related Practice
Textbook Question
Use tabulated electrode potentials to calculate ∆G°rxn for each reaction at 25 °C. a. 2 Fe3+(aq) + 3 Sn(s) → 2 Fe(s) + 3 Sn2+(aq) b. O2(g) + 2 H2O(l) + 2 Cu(s) → 4 OH–(aq) + 2 Cu2+(aq) c. Br2(l) + 2 I–(aq) → 2 Br–(aq) + I2(s)
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Textbook Question
Calculate the equilibrium constant for each of the reactions in Problem 65.
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Open Question
Calculate the equilibrium constant for the reaction between Ni2+(aq) and Cd(s) at 25 °C.
Textbook Question
Calculate the equilibrium constant for the reaction between Fe2+(aq) and Zn(s) (at 25 °C).
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Open Question
Calculate ΔG°_rxn and E°_cell for a redox reaction with n = 2 that has an equilibrium constant of K = 25 (at 25 °C).