What is the equilibrium constant at 298 K for the disproportionation of uranium(V) in acidic solution as shown below? 2 UO2+(aq) + 4 H+(aq) ⇄UO2 2+(aq) + U4+(aq) + 2 H2O(l) Keq = ??? Half-reaction E°, V UO2 2+(aq) + e– → UO2+(aq) +0.16UO2+(aq) + 4 H+(aq) + e– →U4+(aq) + 2 H2O(l)+0.27 (A) 1.9 × 10-4 (B) 73 (C) 5300 (D) 1.9 × 107
What is the equilibrium constant at 298 K for the disproportionation of uranium(V) in acidic solution as shown below? 2 UO2+(aq) + 4 H+(aq) ⇄UO2 2+(aq) + U4+(aq) + 2 H2O(l) Keq = ??? Half-reaction E°, V UO2 2+(aq) + e– → UO2+(aq) +0.16UO2+(aq) + 4 H+(aq) + e– →U4+(aq) + 2 H2O(l)+0.27 (A) 1.9 × 10-4 (B) 73 (C) 5300 (D) 1.9 × 107
General Chemistry - Standalone book (MindTap Course List)
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Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.111QP: a Calculate the equilibrium constant for the following reaction at 25C. Sn(s)+Pb2+(aq)Sn2+(aq)+Pb(s)...
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Question
What is the equilibrium constant at 298 K for the
disproportionation of uranium(V) in acidic solution as
shown below?
2 UO2+(aq) + 4 H+(aq) ⇄UO2 2+(aq) + U4+(aq) + 2 H2O(l)
Keq = ???
Half-reaction E°, V
UO2 2+(aq) + e– → UO2+(aq) +0.16UO2+(aq) + 4 H+(aq) + e– →U4+(aq) + 2 H2O(l)+0.27
(A) 1.9 × 10-4 (B) 73
(C) 5300 (D) 1.9 × 107
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