5.2 redox chemistry 🐂

Question 1

what is disproportionation reaction?

Answer 1

a reaction in which the same element is simultaneously reduced and oxidised to form two different products

Question 2

what is comproportionation reaction?

Answer 2

a reaction in which the two reactants, each containing the same element but with different oxidation state, will form a product in which the element involved reaches the same oxidation state

Question 3

whats the #1 rule in redox!!

Answer 3

amount of electrons lost from oxidation = amount of electrons gained in reduction

Question 4

common oxidising agents (reduced)

Answer 4

• Mn O4- -> Mn2+ (acidic)
• MnO4- -> MnO2 (basic)
• Cr2O7 2- -> Cr3+ (acidic)
• Fe3+ -> Fe2+
• I2 -> 2I-
• SO4 2- -> SO3 2-
• H2O2 -> H2O

Question 5

common reducing agents (oxidised)

Answer 5

• Fe2+ -> Fe3+
• 2I- -> I2
• H2O2 -> O2
• SO3 2- -> SO4 2-

Question 6

why is H2SO4 used to provide acidic medium and not HCl and HNO3?

Answer 6

HCl is not used as the chloride ions will get oxidised by MnO4-.
HNO3 is not used as it is a strong oxidising agent and will interfere with oxidising action of MnO4-