Which species in each pair is a better oxidizing agent under standard-state conditions: (a) Br₂ or Au³+? (b) H₂ or Agt? (c) Cd²+ or Cr³+? (d) O₂ in acidic media or O₂ in basic media?

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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Solve the following queries. Make sure to show complete procedure
a)
Which species in each pair is a better oxidizing agent under standard-state
conditions: (a) Br₂ or Au³+? (b) H₂ or Agt? (c) Cd²+ or Cr³+? (d) O2 in acidic media
or O₂ in basic media?
At equal concentrations of Fe²+ and Fe³+, what must [Ag*] be so that the voltage
b) of the galvanic cell made from the (Ag*|Ag) and (Fe³+|Fe²+) electrodes equals
zero? (b) Determine the equilibrium constant at 25 °C for the reaction under
standard conditions. The reaction for this cell is: Fe²+ +Ag*→Fe³+ +Ag
c)
If H₂O2 is mixed with Fe²+, which reaction is more likely: the oxidation of Fe²+ to
Fe³+ or the reduction of Fe²+ to Fe? In answering, write the reaction for each
possibility and calculate the standard potential of the equivalent electrochemical
cell.
Transcribed Image Text:Solve the following queries. Make sure to show complete procedure a) Which species in each pair is a better oxidizing agent under standard-state conditions: (a) Br₂ or Au³+? (b) H₂ or Agt? (c) Cd²+ or Cr³+? (d) O2 in acidic media or O₂ in basic media? At equal concentrations of Fe²+ and Fe³+, what must [Ag*] be so that the voltage b) of the galvanic cell made from the (Ag*|Ag) and (Fe³+|Fe²+) electrodes equals zero? (b) Determine the equilibrium constant at 25 °C for the reaction under standard conditions. The reaction for this cell is: Fe²+ +Ag*→Fe³+ +Ag c) If H₂O2 is mixed with Fe²+, which reaction is more likely: the oxidation of Fe²+ to Fe³+ or the reduction of Fe²+ to Fe? In answering, write the reaction for each possibility and calculate the standard potential of the equivalent electrochemical cell.
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