- ADehydration reaction
- BOxidation reaction
- ✓Disproportionation reaction
- DDephosphorelation reaction
$4 H _3 PO _3 \rightarrow 3 H _3 PO _4+ PH _3$
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$\left[\Lambda_{\mathrm{m}}=\right.$ molar conductivity
$\Lambda_{\mathrm{m}}^{\circ}=$ limiting molar conductivity
$\mathrm{c}=$ molar concentration
$\mathrm{K}_{\mathrm{a}}=$ dissociation constant of $\mathrm{HX}$ ]

Given $SO_3(g) + H_2O(l) \rightarrow H_2SO_4(l)$
$\Delta H = -130\,\, kcal\, mol^{-1}$
$SO_2(g) + 1/2O_2(g) \rightarrow SO_3(g)$
$\Delta H = -100 \,\,kcal\,\, mol^{-1}$
the enthalpy of formation of $H_2SO_4(l)$ would be ......$kcal\, mol^{-1}$
$S\left( s \right) + {O_2}\left( g \right) \rightleftharpoons S{O_2}\left( g \right);{K_1} = {10^{52}}$
$2S\left( s \right) + 3{O_2}\left( g \right) \rightleftharpoons 2S{O_3}\left( g \right);{K_2} = {10^{129}}$
The equilibrium constant for the reaction $2S{O_2}\left( g \right) + {O_2}\left( g \right) \rightleftharpoons 2S{O_3}\left( g \right)$ is