Consider the Latimer and Frost diagrams for uranium in acidic aqueous solution.

Question

Consider the Latimer and Frost diagrams for uranium in acidic aqueous solution.

Consider the Latimer and Frost diagrams for uranium in acidic aqueous solution. +6 2+ 0.17 V +0.38 V 2+-0.1 V 4 U(s) -6 oxidation state a. What is the most stable state of uranium? b. What are the consequences of dissolving U2+ in aqueous acidic (pH-0) solution? i. Does this reaction proceed by comproportionation or disproportionation? ii. Write a balanced reaction and calculate the electrochemical potential for the reaction. iii. Is the net reaction thermodynamically favorable? Kinetically favorable? b. Calculate the reduction potential for reducing U+ to UO22+ in aqueous acidic solution. Write the balanced equation for this reaction. Calculate the reduction potential for UO22+ at pH-7 c.

Explanation / Answer

a) The species occupying the lowest position in the diagram has the element in its most stable oxidation state ( U4+ )

b) It has been observed that if the point of two species in a frost diagram lies above the line connecting the two adjacent point of two species, it would undergo disproportionation. If the point of a species in a frost diagram lies below the line connecting the two adjacent points of two species, the species will not undergo disproportionation

i) The reactions proceed through disproportionation

ii) Electrochemical potential:

Eo=(1x0.17+1x0.38+1x-0.52+1x-4.7+1x-0.1)/5= -4.77/5= -0.95V

c) Reduction potential for UO2+2 to U4+:

Eo = 1(0.17)+1(0.38)/2= +0.275V

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