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(B) Molar conductivity in aqueous solution depends on the number of ions produced upon dissociation.$(I) K[Co(NH_3)_2(NO_2)_4] \rightarrow K^+ + [Co(N

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$II < I < IV < III$

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(B) Molar conductivity in aqueous solution depends on the number of ions produced upon dissociation.$(I) K[Co(NH_3)_2(NO_2)_4] \rightarrow K^+ + [Co(NH_3)_2(NO_2)_4]^-$. Total ions = $2$.$(II) [Cr(NH_3)_3(NO_2)_3] \rightarrow$ Non-electrolyte. Total ions = $0$ (or $1$ molecule).$(III) [Cr(NH_3)_5NO_2]_3[Co(NO_2)_6]_2 \rightarrow 3[Cr(NH_3)_5NO_2]^{2+} + 2[Co(NO_2)_6]^{3-}$. Total ions = $3 + 2 = 5$.$(IV) Mg[Cr(NH_3)(NO_2)_5] \rightarrow Mg^{2+} + [Cr(NH_3)(NO_2)_5]^{2-}$. Total ions = $2$.Comparing the number of ions: $(III) (5) > (I) = (IV) (2) > (II) (0)$.However,since $(I)$ and $(IV)$ both produce $2$ ions,we look at the charge density. Generally,the order is $(III) > (IV) > (I) > (II)$.Checking the options,option $(B)$ $II < I < IV < III$ is the most appropriate representation of the increasing order.

The correct order of molar conductivity of the following complex compounds in aqueous solution is:
$(I) K[Co(NH_3)_2(NO_2)_4]$
$(II) [Cr(NH_3)_3(NO_2)_3]$
$(III) [Cr(NH_3)_5NO_2]_3[Co(NO_2)_6]_2$
$(IV) Mg[Cr(NH_3)(NO_2)_5]$

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The correct order of molar conductivity of the following complex compounds in aqueous solution is:$(I) K[Co(NH_3)_2(NO_2)_4]$$(II) [Cr(NH_3)_3(NO_2)_3]$$(III) [Cr(NH_3)_5NO_2]_3[Co(NO_2)_6]_2$$(IV) Mg[Cr(NH_3)(NO_2)_5]$