Read the link and answer the questions: bttps//www.ehem.tamu.edu/class/fyp/stone/tuterialnoefiles/electro/nernst. htm Which oes is WRONG about Nemst cquation \( \mathrm{E}=\mathrm{E}^{\circ}-(\mathrm{RT} / \mathrm{nF}) \operatorname{toQ} \) ? A. \( \mathrm{B} \) is cell potential (V) under specific conditions B. \( \mathrm{E}^{0} \) is cell potential at standard-state conditions C. \( \ln Q_{e} \) is the natural log of the reaction quotient at the moment in time D. \( \mathrm{B} \) is the number of half reaction
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Erom the half-reactions below, determine the cell reaction and standard cell potential. $$ \begin{aligned} \mathrm{BrO}_{3}^{-}+6 \mathrm{H}^{+}+6 e^{-} \rightleftharpoons \mathrm{Br}^{-}+3 \mathrm{H}_{2} \mathrm{O} & \\ & E_{\mathrm{BrO}^{-}}^{\circ}=1.44 \mathrm{~V} \\ \mathrm{I}_{2}+2 e^{-} \rightleftharpoons 2 \mathrm{I}^{-} & E_{\mathrm{l}_{2}}^{\circ}=0.54 \mathrm{~V} \end{aligned} $$
56. Consider a voltaic cell in which the following reaction takes place in basic medium at $25^{\circ} \mathrm{C}$. $$ 2 \mathrm{NO}_{3}^{-}(a q)+3 \mathrm{~S}^{2-}(a q)+4 \mathrm{H}_{2} \mathrm{O} \longrightarrow 3 \mathrm{~S}(s)+2 \mathrm{NO}(g)+8 \mathrm{OH}^{-}(a q) $$ (a) Calculate $E^{\circ}$. (b) Write the Nernst equation for the cell voltage $E$. (c) Calculate $E$ under the following conditions: $P_{\mathrm{NO}}=0.994 \mathrm{~atm},$ $\mathrm{pH}=13.7,\left[\mathrm{~S}^{2-}\right]=0.154 \mathrm{M},\left[\mathrm{NO}_{3}^{-}\right]=0.472 \mathrm{M}$
Consider the voltaic cell at $25^{\circ} \mathrm{C}$ in which the following reaction takes place: $$ \mathrm{MnO}_{2}(s)+4 \mathrm{H}^{+}(a q)+2 \mathrm{Br}^{-}(a q) \longrightarrow_{\mathrm{Br}_{2}(l)}+\mathrm{Mn}^{2+}(a q)+2 \mathrm{H}_{2} \mathrm{O} $$ (a) Calculate $E^{\circ}$. (b) Write the Nernst equation for the cell. (c) Find $E$ under the following conditions: $\left[\mathrm{Mn}^{2+}\right]=$ $0.60 \mathrm{M},\left[\mathrm{Br}^{-}\right]=0.83 \mathrm{M}, \mathrm{pH}=3.17$
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