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Consider the half-reaction below with an E° value of –2.069 V:
[AlF6]3–(aq) + 3 e– → Al(s) + 6 F–(aq)
Determine the formation constant (Kf) of [AlF6]3–. [Use E°red Al3+ = –1.662 V]
Identify whether the following statement is True or False: The value of ΔG° will be positive and K will be less than 1 when a reaction has a positive E° value.
Given the following E°red
Cl2(g) + 2 e− → 2 Cl− (aq) E°red = 1.36 V
MnO4−(aq) + 8 H+(aq) + 5 e− → Mn2+(aq) + 4 H2O(l) E°red = 1.51 V
What is the value of the equilibrium constant for the reaction at 298 K?
10 Cl− (aq) + 2 MnO4−(aq) + 16 H+(aq) → 2 Mn2+(aq) + 8 H2O(l) + 5 Cl2(g)
Predict the sign of E° when K > 1 and determine the value of K if E° = 0 V.
Consider the reaction of Cu2+(aq) and Ni(s) at 25 °C. Calculate the equilibrium constant for this reaction using reduction potentials.
A cell reaction has a reading of 2.1 V at 298 K. What is the value of n if the reaction has an equilibrium constant of 3.289 × 1035?