MCQ
In neutral or alkaline solution, $MnO _{4}^{-}$oxidises thiosulphate to.
- A$S _{2} O _{7}^{2-}$
- B$S _{2} O _{8}^{2-}$
- C$SO _{3}^{2-}$
- ✓$SO _{4}^{2-}$
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$(A)\xrightarrow{{\operatorname{Re}duction}}(B)\xrightarrow{{HN{O_2}}}{C_2}{H_5}OH$
In the above first order reaction the initial concentration of $\mathrm{N}_{2} \mathrm{O}_{5}$ is $2.40 \times 10^{-2}\, \mathrm{~mol} \,\mathrm{~L}^{-1}$ at $318 \,K.$ The concentration of $\mathrm{N}_{2} \mathrm{O}_{5}$ after $1\, hour$ was $1.60 \times 10^{-2}\, \mathrm{~mol} \,\mathrm{~L}^{-1}$, The rate constant of the reaction at $318\, \mathrm{~K}$ is $.....\,\times 10^{-3} \mathrm{~min}^{-1}$. (Nearest integer)
[Given: $\log 3=0.477, \log 5=0.699$ ]