Electrochemistry · Nernst equation cell EMF

Consider the following electrochemical cell at 298K

$\mathrm{Pt}\,|\,\ce{HSnO2^-}(\mathrm{aq})\,|\,\ce{Sn(OH)6^{2-}}(\mathrm{aq})\,|\,\ce{Bi2O3}(\mathrm{s})\,|\,\mathrm{Bi}(\mathrm{s})$.

If the reaction quotient at a given time is $10^{6}$, then the cell EMF ($E_\mathrm{cell}$) is $\times\,10^{-1}$ V (Nearest integer).

Given the standard half-cell reduction potential as

$E^{0}_{\ce{Bi2O3}/\mathrm{Bi},\,\ce{OH-}} = -0.44$ V and

$E^{0}_{\ce{Sn(OH)6^{2-}}/\ce{HSnO2^-},\,\ce{OH-}} = -0.90$ V