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Consider the Latimer diagram for phosphorus in acidic and basic solutions at 25 °C.

Consider the Latimer diagram for phosphorus in acidic and basic solutions at 25 °C.

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 74QAP: Consider the reaction low at 25°C: 3SO42(aq)+12H+(aq)+2Cr(s)3SO2(g)+2Cr3+(aq)+6H2O Use Table 17.1 to...
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2. Consider the Latimer diagram for phosphorus in acidic and basic solutions at 25 °C. Acidic solution H3PO4 -0.93 Basic solution PO4³- H4P₂O6 -0.28 a HPO3²- -1.35 H3PO3 -1.49 -1.57 b H₂PO₂ H₂PO₂2 -0.50 y -0.51 P -1.18 -0.06 PH3 PH3 A. Complete the missing standard reduction potentials (a, b and c) for the Latimer diagram in acidic solution. B. Complete the missing standard reduction potentials (x, y and z) for the Latimer diagram in basic solution. C. Consider the redox reaction shown below in basic solution at 25 °C. HPO32- (aq) )+ PH3(g) ₹ 2 P(s) + 2 OH (aq) + H₂O(1) (i) Write the balanced equation for the cathode half-reaction and calculate the Eºred- (ii) Write the balanced equation for the anode half-reaction and calculate the Eºox. (iii) Calculate the Eᵒcell and AG for the given redox reaction.
Transcribed Image Text:2. Consider the Latimer diagram for phosphorus in acidic and basic solutions at 25 °C. Acidic solution H3PO4 -0.93 Basic solution PO4³- H4P₂O6 -0.28 a HPO3²- -1.35 H3PO3 -1.49 -1.57 b H₂PO₂ H₂PO₂2 -0.50 y -0.51 P -1.18 -0.06 PH3 PH3 A. Complete the missing standard reduction potentials (a, b and c) for the Latimer diagram in acidic solution. B. Complete the missing standard reduction potentials (x, y and z) for the Latimer diagram in basic solution. C. Consider the redox reaction shown below in basic solution at 25 °C. HPO32- (aq) )+ PH3(g) ₹ 2 P(s) + 2 OH (aq) + H₂O(1) (i) Write the balanced equation for the cathode half-reaction and calculate the Eºred- (ii) Write the balanced equation for the anode half-reaction and calculate the Eºox. (iii) Calculate the Eᵒcell and AG for the given redox reaction.
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