(Solved): please answer i will leave a thumbs up!! A galvanic cell consists of the following half-reactions An ...

A galvanic cell consists of the following half-reactions Anode: \( A(s) \rightarrow A^{3+}(\mathrm{aq})+3 e^{-} E^{0} \) ox \( =0.50 \) Cathode: \( B^{+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{B}(\mathrm{s}) \quad \mathrm{E}_{\text {red }}^{\mathrm{O}}=1.02 \) The cells are connected at \( 25^{\circ} \mathrm{C} \). The concentration of \( \mathrm{A}^{3+} \) is \( 0.73 \mathrm{M} \), while the concentration of \( \mathrm{B}^{+} \) is \( 0.032 \mathrm{M} \). Use the Nernst equationIto determine the cell potential in volts of this non-standard cell. Report your answer to two places after the decimal QUESTION 2 Given the following reaction at \( 25^{\circ} \mathrm{C} \) \[ 3 A(s)+2 B^{3+}(\mathrm{aq}) \rightarrow 3 A^{2+}(\mathrm{aq})+2 \mathrm{~B}(\mathrm{~s}), E^{0}=0.16 \] Determine the equilibrium constant, \( \mathrm{K} \) for this reaction. Report your answer in scientific notation. \( 1.2 \times 10^{3} \) would be entered as \( 1.2 \mathrm{E} 3 \) with no spaces.