Balance the following equations in basic medium by ion electron and oxidation number methods and identify the oxidising agent and the reducing agent
\(CI_{ 2 }O_{ 7 }(g)+H_{ 2 }O_{ 2 }(aq)\longrightarrow CIO_{ 2 }^{ - }(aq)+O_{ 2 }(g)\)

2

(a)

A solution of silver nitrate was stirred with iron rod.Will it cause any change in the concentration of silver and nitrate ions?

2

(a)

How many millimoles of potassium dichromate is required to oxidise 24mL of 0.5 M Mohr's salt solution in acidic medium?

2

(a)

Two half cells are AI³⁺ (aq) /AI and Mg²⁺ (aq)/Mg.The reduction potentials of these half-cells are -1.66 V and -2.36 V respectively. Calculate the cell potential. Write the cell reaction also. 

2

(a)

Assign oxidation number to the underlined elements in each of the following species - K₂MnO₄

2

(a)

What are the oxidation numbers of the underlined elements and how do you rationalise your results? CH₃COOH

2

(a)

Fluorine reacts with ice and results in the change: H₂O(s) + F2(g) \(\rightarrow\) HF(g) + HOF(g) justify that this reaction is a redox reaction.

2

(a)

What is a redox couple?

2

(a)

Define oxidation in terms of electronic concept

2

(a)

What is the oxidation state of Ni in Ni (CO)₄

2

(a)

What is the oxidation number of P in H₃PO₄?

2

(a)

Why is standard hydrogen electrode called reversible electrode?

2

(a)

Calculate the oxidation number of sulphur in H2_SO₄ and Na₂SO₄

2

(a)

Define Oxidation and Reduction in terms of oxidation number.

2

(a)

In the reaction M₄O₂ + 4HCl \(\rightarrow\) M₄Cl_{2 +} Cl₂+2H₂O Which species is oxidised

2

(a)