The oxidation of HNO2 to NO3 in acid solution is a 4-electron transfer reaction described by the following equation: 2HNO₂ (aq) + 0₂ (8) 2NO3(aq) +2H+ (aq) E° cell = 0.289 V If the reaction at 298 K is in equilibrium with air (Po2 = 0.150 atm) at pH 5.60, what is the ratio of [NO3] to [HNO₂]?

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Chapter18: Electrochemistry
Section: Chapter Questions
Problem 88E: For the following half-reaction, = 2.07 V: A1F63(aq)+3eAl(s)+6F(aq) Using data from Table 17-1,...
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The oxidation of HNO2 to NO3¯ in acid solution is a 4-electron transfer reaction described by the following equation:
2HNO₂ (aq) +O₂(g)
=
→ 2NO3 (aq) +2H¹ (aq) E cell
0.289 V
If the reaction at 298 K is in equilibrium with air (Po2 = 0.150 atm) at pH 5.60, what is the ratio of [NO3¯] to [HNO₂]?
Transcribed Image Text:The oxidation of HNO2 to NO3¯ in acid solution is a 4-electron transfer reaction described by the following equation: 2HNO₂ (aq) +O₂(g) = → 2NO3 (aq) +2H¹ (aq) E cell 0.289 V If the reaction at 298 K is in equilibrium with air (Po2 = 0.150 atm) at pH 5.60, what is the ratio of [NO3¯] to [HNO₂]?
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