KCET 2025 | Redox Reactions Question 1 | Chemistry

List-I (Types of redox reactions)	List-II (Examples)
a. Combination reaction	i. ${Cl}_{2 (g)} + 2 {Br}_{(aq)}^{-} \to 2 {Cl}_{(aq)}^{-} + {Br}_{2 (1)}$
b. Decomposition reaction	ii. $2 H_{2} O_{2 (aq)} \to 2 H_{2} O_{(l)} + O_{2 (g)}$
c. Displacement reaction	iii. ${CH}_{4 (g)} + 2 O_{2 (g)} \overset{Δ}{\to} {CO}_{2 (g)} + 2 H_{2} O_{(l)}$
d. Disproportionation reaction	iv. $2 H_{2} O_{(1)} \overset{Δ}{\to} 2 H_{2 (g)} + O_{2 (g)}$

$$ \text { Choose the correct answer from the options given below. } $$

a-iv, b-iii, c-i, d-ii

a-ii, b-i, c-iv, d-iii

a-iii, b-iv, c-i, d-ii

a-iii, b-ii, c-i, d-iv

KCET 2025

MCQ (Single Correct Answer)

-0

In the reaction between hydrogen sulphide and acidified permanganate solution,

$\mathrm{H}_2 \mathrm{~S}$ is reduced to $\mathrm{S}, \mathrm{MnO}_4^{-}$is oxidised to $\mathrm{Mn}^{2+}$

$\mathrm{H}_2 \mathrm{~S}$ is oxidised to $\mathrm{SO}_2, \mathrm{MnO}_4^{-}$is reduced to $\mathrm{MnO}_2$

$\mathrm{H}_2 \mathrm{~S}$ is reduced to $\mathrm{SO}_2, \mathrm{MnO}_4^{-}$is oxidised to $\mathrm{Mn}^{2+}$

$\mathrm{H}_2 \mathrm{~S}$ is oxidised to $\mathrm{S}, \mathrm{MnO}_4^{-}$is reduced to $\mathrm{Mn}^{2+}$

KCET 2025

MCQ (Single Correct Answer)

-0

In the titration of potassium permanganate $\left(\mathrm{KMnO}_4\right)$ against Ferrous ammonium sulphate $(\mathrm{FAS})$ solution, dilute sulphuric acid but not nitric acid is used to maintain acidic medium, because

It is difficult to identify the end point

Nitric acid doesn't act as an indicator

Nitric acid itself is an oxidizing agent

Nitric acid is a weak acid than sulphuric acid

KCET 2024

MCQ (Single Correct Answer)

-0

In the reaction between moist $\mathrm{SO}_2$ and acidified permanganate solution.

$\mathrm{SO}_2$ is oxidised to $\mathrm{SO}_4^{2-}$. $\mathrm{MnO}_4^{-}$is reduced to $\mathrm{Mn}^{2+}$.

$\mathrm{SO}_2$ is reduced to S . $\mathrm{MnO}_4^{-}$is oxidised to $\mathrm{MnO}_4$.

$\mathrm{SO}_2$ is oxidised to $\mathrm{SO}_3^{2-}$. $\mathrm{MnO}_4^{-}$is reduced to $\mathrm{MnO}_2$.

$\mathrm{SO}_2$ is reduced to $\mathrm{H}_2 \mathrm{~S}$. $\mathrm{MnO}_4^{-}$is oxidised to $\mathrm{MnO}_4$.

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