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
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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.
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