hi!
can someone help me solve this q from hsc 2012
thank you!
13) First of all, remember that the
oxidising agent does the oxidising, so is being reduced. This means that the oxidising agent has to be on the reactants side, so this gets rid of B. Also note that a substance is being reduced when its oxidation state
reduces.
Let's look at the oxidation states of the others
A) H
+: +1 at first, and stays at +1 in water
C) Fe
2+: +2 at first, +3 after. Iron is being oxidised, so the answer isn't c)
D) Cr
2O
72-: Looking at Cr, +6 at first (let me know if you don't understand how I got this), +3 after! So it has been reduced, therefore it is the oxidising agent and the answer is D
14) So the oxidation and reduction eqns are:
Oxidation: 6Fe
2+ <--> 6Fe
3++6e
-E
oxidation= -0.77 V (remember to change the sign for oxidation when using the values on the data sheet)
Reduction: Cr
2O
72-+14H
++6e
- <--> 2Cr
3+ + 7H
2O
E
reduction= 1.36V
Therefore E
total= 1.36 - 0.77 = 0.59 V! So the answer is A