Choose the spontaneous direction for the following reaction: \[ \mathrm{Co}+\mathrm{Ga}^{3+} \longleftrightarrow \mathrm{Ga}+\mathrm{Co}^{2+} \] Calculate \( E^{\circ} \) for the spontaneous direction. Calculate \( \Delta G^{\circ} \) and \( \mathrm{k} \) for the spontaneous reaction. If the concentration of \( \mathrm{Ga}^{3+} \) is \( .26 \mathrm{M} \) and the concentration of \( \mathrm{Co}^{2+} \) is \( .15 \mathrm{M} \), what is your \( \mathrm{E} \) value? If you ran this battery at 2.3 amps for 23 minutes, what would be the new \( \mathrm{E} \) for this battery?
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The half-reaction with the higher reduction potential will proceed as a reduction (gain of electrons), while the other half-reaction will proceed as an oxidation (loss of electrons). The standard reduction potentials for Co and Ga are as follows: Co^2+ + 2e^- Show more…
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Under standard conditions for all concentrations, the following reaction is spontaneous at $25^{\circ} \mathrm{C}$. $$ \begin{aligned} \mathrm{O}_{3}(g)+2 \mathrm{H}^{+}(a q)+2 \mathrm{Co}^{2+}(a q) & \longrightarrow \\ \mathrm{O}_{2}(g) &+\mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{Co}^{3+}(a q) \end{aligned} $$ If $\left[\mathrm{H}^{+}\right]$ is decreased so that the $\mathrm{pH}=9.00$, what value will $E_{\text {cell }}$ have, and will the reaction be spontaneous at this $\left[\mathrm{H}^{+}\right] ?$
Calculate the free energy change for this reaction at $25^{\circ} \mathrm{C}$ . Is the reaction spontaneous? (Assume that all reactants and products are in their standard states.) $$\begin{array}{c}{\mathrm{C}_{3} \mathrm{H}_{8}(g)+5 \mathrm{O}_{2}(g) \longrightarrow 3 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)} \\ {\Delta H_{\mathrm{rxn}}^{\circ}=-2217 \mathrm{kJ} ; \Delta S_{\mathrm{rxn}}^{\circ}=101.1 \mathrm{J} / \mathrm{K}}\end{array}$$
Determine whether the following redox reaction is spontaneous at $25^{\circ} \mathrm{C}$ and 1 atm: $$2 \mathrm{KIO}_{3}(s)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{KClO}_{3}(s)+\mathrm{I}_{2}(s)$$ Use data in Appendix 1 and the following information: $\Delta H_{\mathrm{f}}^{\circ} \mathrm{KIO}_{3}(s)=$ $-501.4 \mathrm{~kJ} / \mathrm{mol}, \mathrm{S}^{\circ} \mathrm{KIO}_{3}(s)=151.5 \mathrm{~J} / \mathrm{mol} \cdot \mathrm{K} .$ What is the lowest temperature at which the reaction is spontaneous?
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