330086 A standard hydrogen electrode has a zero potential because

330087 Deduce from the following \(\mathrm{E}^{\circ}\) values of half cells, what combination of two half cells would result in a cell with the largest potential?
I. \(\mathrm{A} \rightarrow \mathrm{A}^{+}+\mathrm{e} ; \mathrm{E}^{\circ}=-0.24 \mathrm{~V}\)
II. \(\mathrm{B}^{+} \rightarrow \mathrm{B}+\mathrm{e} ; \mathrm{E}^{\circ}=-2.1 \mathrm{~V}\)
III. \(\mathrm{C} \rightarrow \mathrm{C}^{2+}+2 \mathrm{e}^{-} ; \mathrm{E}^{0}=-0.38 \mathrm{~V}\)
IV. \(\mathrm{D}^{2-} \rightarrow \mathrm{D}^{-}+\mathrm{e}^{-} ; \mathrm{E}^{0}=-0.59 \mathrm{~V}\)

330088 For the cell reaction, \(2{\text{C}}{{\text{e}}^{4 + }} + {\text{Co}} \to 2{\text{C}}{{\text{e}}^{3 + }}{\text{C}}{{\text{o}}^{2 + }};\,\,{\text{E}}{^\circ _{{\text{cell}}}}{\text{is}}\,\,1.89\,{\text{V}}.\) if \({{\text{E}}_{{\text{C}}{{\text{o}}^{2 + }}/{\text{Co}}}}{\mkern 1mu} {\mkern 1mu} \) is \({\mkern 1mu} - 0.28{\text{V}},\) What is the value of \({\text{E}}{^\circ _{{\text{C}}{{\text{e}}^{{\text{4 + }}}}{\text{/}}\,\,{\text{C}}{{\text{e}}^{{\text{3 + }}}}}}\)?

330089 Which cell will measure standard electrode potential of copper electrode?

330086 A standard hydrogen electrode has a zero potential because

330087 Deduce from the following \(\mathrm{E}^{\circ}\) values of half cells, what combination of two half cells would result in a cell with the largest potential?
I. \(\mathrm{A} \rightarrow \mathrm{A}^{+}+\mathrm{e} ; \mathrm{E}^{\circ}=-0.24 \mathrm{~V}\)
II. \(\mathrm{B}^{+} \rightarrow \mathrm{B}+\mathrm{e} ; \mathrm{E}^{\circ}=-2.1 \mathrm{~V}\)
III. \(\mathrm{C} \rightarrow \mathrm{C}^{2+}+2 \mathrm{e}^{-} ; \mathrm{E}^{0}=-0.38 \mathrm{~V}\)
IV. \(\mathrm{D}^{2-} \rightarrow \mathrm{D}^{-}+\mathrm{e}^{-} ; \mathrm{E}^{0}=-0.59 \mathrm{~V}\)

330088 For the cell reaction, \(2{\text{C}}{{\text{e}}^{4 + }} + {\text{Co}} \to 2{\text{C}}{{\text{e}}^{3 + }}{\text{C}}{{\text{o}}^{2 + }};\,\,{\text{E}}{^\circ _{{\text{cell}}}}{\text{is}}\,\,1.89\,{\text{V}}.\) if \({{\text{E}}_{{\text{C}}{{\text{o}}^{2 + }}/{\text{Co}}}}{\mkern 1mu} {\mkern 1mu} \) is \({\mkern 1mu} - 0.28{\text{V}},\) What is the value of \({\text{E}}{^\circ _{{\text{C}}{{\text{e}}^{{\text{4 + }}}}{\text{/}}\,\,{\text{C}}{{\text{e}}^{{\text{3 + }}}}}}\)?

330089 Which cell will measure standard electrode potential of copper electrode?

330086 A standard hydrogen electrode has a zero potential because

330087 Deduce from the following \(\mathrm{E}^{\circ}\) values of half cells, what combination of two half cells would result in a cell with the largest potential?
I. \(\mathrm{A} \rightarrow \mathrm{A}^{+}+\mathrm{e} ; \mathrm{E}^{\circ}=-0.24 \mathrm{~V}\)
II. \(\mathrm{B}^{+} \rightarrow \mathrm{B}+\mathrm{e} ; \mathrm{E}^{\circ}=-2.1 \mathrm{~V}\)
III. \(\mathrm{C} \rightarrow \mathrm{C}^{2+}+2 \mathrm{e}^{-} ; \mathrm{E}^{0}=-0.38 \mathrm{~V}\)
IV. \(\mathrm{D}^{2-} \rightarrow \mathrm{D}^{-}+\mathrm{e}^{-} ; \mathrm{E}^{0}=-0.59 \mathrm{~V}\)

330088 For the cell reaction, \(2{\text{C}}{{\text{e}}^{4 + }} + {\text{Co}} \to 2{\text{C}}{{\text{e}}^{3 + }}{\text{C}}{{\text{o}}^{2 + }};\,\,{\text{E}}{^\circ _{{\text{cell}}}}{\text{is}}\,\,1.89\,{\text{V}}.\) if \({{\text{E}}_{{\text{C}}{{\text{o}}^{2 + }}/{\text{Co}}}}{\mkern 1mu} {\mkern 1mu} \) is \({\mkern 1mu} - 0.28{\text{V}},\) What is the value of \({\text{E}}{^\circ _{{\text{C}}{{\text{e}}^{{\text{4 + }}}}{\text{/}}\,\,{\text{C}}{{\text{e}}^{{\text{3 + }}}}}}\)?

330089 Which cell will measure standard electrode potential of copper electrode?

330086 A standard hydrogen electrode has a zero potential because

330087 Deduce from the following \(\mathrm{E}^{\circ}\) values of half cells, what combination of two half cells would result in a cell with the largest potential?
I. \(\mathrm{A} \rightarrow \mathrm{A}^{+}+\mathrm{e} ; \mathrm{E}^{\circ}=-0.24 \mathrm{~V}\)
II. \(\mathrm{B}^{+} \rightarrow \mathrm{B}+\mathrm{e} ; \mathrm{E}^{\circ}=-2.1 \mathrm{~V}\)
III. \(\mathrm{C} \rightarrow \mathrm{C}^{2+}+2 \mathrm{e}^{-} ; \mathrm{E}^{0}=-0.38 \mathrm{~V}\)
IV. \(\mathrm{D}^{2-} \rightarrow \mathrm{D}^{-}+\mathrm{e}^{-} ; \mathrm{E}^{0}=-0.59 \mathrm{~V}\)

330088 For the cell reaction, \(2{\text{C}}{{\text{e}}^{4 + }} + {\text{Co}} \to 2{\text{C}}{{\text{e}}^{3 + }}{\text{C}}{{\text{o}}^{2 + }};\,\,{\text{E}}{^\circ _{{\text{cell}}}}{\text{is}}\,\,1.89\,{\text{V}}.\) if \({{\text{E}}_{{\text{C}}{{\text{o}}^{2 + }}/{\text{Co}}}}{\mkern 1mu} {\mkern 1mu} \) is \({\mkern 1mu} - 0.28{\text{V}},\) What is the value of \({\text{E}}{^\circ _{{\text{C}}{{\text{e}}^{{\text{4 + }}}}{\text{/}}\,\,{\text{C}}{{\text{e}}^{{\text{3 + }}}}}}\)?

330089 Which cell will measure standard electrode potential of copper electrode?