330437 For the cell reaction,
\(\mathrm{Cu}^{2+}\left(\mathrm{C}_{1}\right)(\mathrm{aq})+\mathrm{Zn}(\mathrm{s}) \rightarrow \mathrm{Zn}^{2+}\left(\mathrm{C}_{2}\right)\)
\((\mathrm{aq})+\mathrm{Cu}(\mathrm{s})\) of an electrochemical cell, the change in free energy \(\Delta \mathrm{G}\) at a given temperature is a function of

330438 The \(\mathrm{E}^{\circ}\) in the given figure is :

330439 The equilibrium constant of the reaction,
\({\rm{Cu(s)}} + 2{\rm{A}}{{\rm{g}}^ + }({\rm{aq}}) \to {\rm{C}}{{\rm{u}}^{2 + }}({\rm{aq}}) + 2{\rm{Ag(s)}}\)
\({\rm{E}}^\circ {\rm{ }} = 0.46\,{\rm{V}}\,{\rm{at}}{\mkern 1mu} \,298\;{\rm{K}}\,is\)

330440 The standard emf of galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the reaction of the cell is

330437 For the cell reaction,
\(\mathrm{Cu}^{2+}\left(\mathrm{C}_{1}\right)(\mathrm{aq})+\mathrm{Zn}(\mathrm{s}) \rightarrow \mathrm{Zn}^{2+}\left(\mathrm{C}_{2}\right)\)
\((\mathrm{aq})+\mathrm{Cu}(\mathrm{s})\) of an electrochemical cell, the change in free energy \(\Delta \mathrm{G}\) at a given temperature is a function of

330438 The \(\mathrm{E}^{\circ}\) in the given figure is :

330439 The equilibrium constant of the reaction,
\({\rm{Cu(s)}} + 2{\rm{A}}{{\rm{g}}^ + }({\rm{aq}}) \to {\rm{C}}{{\rm{u}}^{2 + }}({\rm{aq}}) + 2{\rm{Ag(s)}}\)
\({\rm{E}}^\circ {\rm{ }} = 0.46\,{\rm{V}}\,{\rm{at}}{\mkern 1mu} \,298\;{\rm{K}}\,is\)

330440 The standard emf of galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the reaction of the cell is

330437 For the cell reaction,
\(\mathrm{Cu}^{2+}\left(\mathrm{C}_{1}\right)(\mathrm{aq})+\mathrm{Zn}(\mathrm{s}) \rightarrow \mathrm{Zn}^{2+}\left(\mathrm{C}_{2}\right)\)
\((\mathrm{aq})+\mathrm{Cu}(\mathrm{s})\) of an electrochemical cell, the change in free energy \(\Delta \mathrm{G}\) at a given temperature is a function of

330438 The \(\mathrm{E}^{\circ}\) in the given figure is :

330439 The equilibrium constant of the reaction,
\({\rm{Cu(s)}} + 2{\rm{A}}{{\rm{g}}^ + }({\rm{aq}}) \to {\rm{C}}{{\rm{u}}^{2 + }}({\rm{aq}}) + 2{\rm{Ag(s)}}\)
\({\rm{E}}^\circ {\rm{ }} = 0.46\,{\rm{V}}\,{\rm{at}}{\mkern 1mu} \,298\;{\rm{K}}\,is\)

330440 The standard emf of galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the reaction of the cell is

330437 For the cell reaction,
\(\mathrm{Cu}^{2+}\left(\mathrm{C}_{1}\right)(\mathrm{aq})+\mathrm{Zn}(\mathrm{s}) \rightarrow \mathrm{Zn}^{2+}\left(\mathrm{C}_{2}\right)\)
\((\mathrm{aq})+\mathrm{Cu}(\mathrm{s})\) of an electrochemical cell, the change in free energy \(\Delta \mathrm{G}\) at a given temperature is a function of

330438 The \(\mathrm{E}^{\circ}\) in the given figure is :

330439 The equilibrium constant of the reaction,
\({\rm{Cu(s)}} + 2{\rm{A}}{{\rm{g}}^ + }({\rm{aq}}) \to {\rm{C}}{{\rm{u}}^{2 + }}({\rm{aq}}) + 2{\rm{Ag(s)}}\)
\({\rm{E}}^\circ {\rm{ }} = 0.46\,{\rm{V}}\,{\rm{at}}{\mkern 1mu} \,298\;{\rm{K}}\,is\)

330440 The standard emf of galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the reaction of the cell is