Question

PLEASE SHOW ME YOUR STEPS!!

Consider the following unbalanced redox equations: a. I

Answer 1

Rules for balancing of equation in ion electrode method:

(1) Identify the species that are oxidized and reduced.

(2) Divide the equation into oxidation half reaction & reduction half reaction

(3) Balance the atoms & charges in each half reaction separately according to the following rules:

(a) First balance the atoms other than that of Hydrogen & Oxygen

(b) Oxygen atoms are balanced by adding the required no. of H₂O molecules to the side deficient in Oxygen atoms:

(c) Then balance Hydrogen atoms. For this

(i)If the reaction is in acidic medium add the required number of H⁺ ions to the side deficient in H atoms

(ii) If the reaction is in basic medium add the required number of H₂O molecules to the side deficient in H atoms and then number of OH^- ions to the other side.

(4) Add required number of electrons to balance the charges

(5) Equalize the number of electrons in the half reactions by multiplying each equation with the required number.

(6) Add the two reactions. so that cancel off the electrons takes place

Calculate the net number of common terms and write down on the proper side.

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Reducing agent is one that it reduces other & oxidizes it-self.So the oxidation state increases for reducing agent.

Oxidizing agent is one that it oxidizes other & reduce it-self.So the oxidation state decreases for oxidizing agent.

-1          +5                 +2         0

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