Question

standard electrode potentials of redox couples
82+/B. C/C2+ and D2+/D are 0.3 V, -0.5 V.
75 V and 0.9 V respectively. Which of these is
hest oxidising agent and reducing agent respectively
(1) D2#/D and B2/B
2) B2/B and D2/D
(3) D2/D and C2+/C
4) C2#/C and D2+/D​



use the attachment

Answer 1

Answer:

Explanation:

Answer is (1)

See

Basically we have ∆G= -nFE°

Now for best oxidising agent see that which one is having more negative value of ∆G

i.e oxidising means it undergoes reduction, so we should see M(+2) to M E° values must be positive

i.e ∆G is more negative for D+2 to D since it have positive E° value

In same way for reduction process.

See M to M+2 that must be positive so that ∆G is negative

So B+2 to B is having positive E° value that means ∆G is negative

∆G negative represents spontaneous reaction is taking place.