MCQ
When $KMn{O_4}$ reacts with acidified $FeS{O_4}$
- AOnly $FeS{O_4}$ is oxidised
- BOnly $KMn{O_4}$ is oxidised
- ✓$FeS{O_4}$ is oxidised $KMn{O_4}$ and is reduced
- DNone of these
$2KMn{O_4} + 3{H_2}S{O_4}\, \to \,{K_2}S{O_4} + 2MnS{O_4}$
$[2FeS{O_4} + {H_2}S{O_4}\, \to \,F{e_2}{(S{O_4})_3} + 2H] \times 5$
$[2H + [O]\, \to \,{H_2}O] \times 5$
$\overline {2KMn{O_4} + 8{H_2}S{O_4} + 10FeS{O_4}{\mkern 1mu} \to } $
${K_2}S{O_4} + 2MnS{O_4} + 5F{e_2}{(S{O_4})_3} + 8{H_2}O$
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$(i)$ $X + Y \rightleftharpoons M$ very rapid equilibrium
$(ii)$ $M + Z \to P$ slow
$(iii)$ $O + Y \to N$ very fast
What is the rate law for this reaction
$[\Lambda_{\mathrm{H}^{+}}^{\circ}=350 \,\mathrm{~S}\, \mathrm{~cm}^{2}\, \mathrm{~mol}^{-1},\Lambda_{\mathrm{CH}_{3} \mathrm{COO}^{-}}^{\circ}=50\, \mathrm{~S}\, \mathrm{~cm}^{2}\, \mathrm{~mol}^{-1}]$
$A$. The stability of the hydrides decreases in the order $\mathrm{NH}_3>\mathrm{PH}_3>\mathrm{AsH}_3>\mathrm{SbH}_3>\mathrm{BiH}_3$
$B$. The reducing ability of the hydrides increases in the order $\mathrm{NH}_3<\mathrm{PH}_3<\mathrm{AsH}_3<\mathrm{SbH}_3<\mathrm{BiH}_3$
$C$. Among the hydrides, $\mathrm{NH}_3$ is strong reducing agent while $\mathrm{BiH}_3$ is mild reducing agent.
$D$. The basicity of the hydrides increases in the order $\mathrm{NH}_3<\mathrm{PH}_3<\mathrm{AsH}_3<\mathrm{SbH}_3<\mathrm{BiH}_3$Choose the most appropriate from the option given below:
$A$ is
The rate of reaction when the concentration of $A$ is $0.01\, M$ is ............$\times 10^{-4}\,M/ \min$