Question

hich species in each pair is a better oxidizing agent under standard-state conditions? a. Br2 or Au3+ b. H2 or Ag+ c. Cd2+ or Cr3+ d. O2 in acidic media or O2 in basic media

Answer 1

Step-by-step explanation:

It is known that species with higher value of reduction potential will act as a good oxidizing agent.

(a) Here we are given
`Br_(2)` and
`Au^(3+)`. Reduction potential of
`Br_(2)` is 1.07 V and reduction potential of
`Au^(3+)` is 1.50 V.

As
`Au^(3+)` has higher value of reduction potential. Hence,
`Au^(3+)` acts as a better oxidizing agent than
`Br_(2)`.

(b) Here we are given
`H_(2)` and
`Ag^(+)`. Reduction potential of
`H_(2)` is 0.00 V and reduction potential of
`Ag^(+)` is 0.80 V.

As
`Ag^(+)` has higher value of reduction potential. Hence,
`Ag^(+)` acts as a better oxidizing agent than
`H_(2)`.

(c) Here we are given
`Cd^(2+)` and
`Cr^(3+)`. Reduction potential of
`Cd^(2+)` is -0.40 V and reduction potential of
`Cr^(3+)` is -0.74 V.

As
`Cd^(2+)` has higher value of reduction potential than
`Cr^(3+)`. Hence,
`Cd^(2+)` acts as a better oxidizing agent.

(d) The given species are
`O_(2)` in acidic medium and
`O_(2)` in basic medium. Reduction potential of
`O_(2)` in acidic medium is 1.23 V and reduction potential of
`O_(2)` in basic medium is 0.40 V.

Thus, we can conclude that
`O_(2)` in acidic medium is better oxidizing agent that
`O_(2)` in basic medium.