First slide

Classical idea of redox reactions

Question

Which of the following reactions is not a redox reaction?

Easy

A

$H_{2} O_{2} + KOH ⟶ {KHO}_{2} + H_{2} O$
B

${Cr}_{2} {O_{7}}^{2 -} + 2 \overset{⊝}{O} H ⟶ 2 {CrO}_{4}^{2 -} + H_{2} O$
C

$Ca {({HCO}_{3})}_{2} \overset{Δ}{⟶} {CaCO}_{3} + {CO}_{2} + H_{2} O$
D

$H_{2} O_{2} ⟶ H_{2} O + \frac{1}{2} O_{2}$

Solution

Oxidation state of K is +1 in both reactant and product.
In (2), oxidation state of Cr(+6) does not change.
In (3) oxidation states of Ca and C and O do not change.
In (4), the H₂O₂ which disproportionates is both oxidasing and a reducing agent.

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