330441 Match the columns.
Given: \(\left(\mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{\circ}=0.8, \mathrm{~K}_{\mathrm{sp}}(\mathrm{AgCl})=10^{-10}\right)\)

330442 The standard emf of a galvanic cell involving 2 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the redox reaction of the cell is

330443 For a cell involving two electron changes,
\({\rm{E}}_{{\rm{cell}}}^{\rm{o}}{\rm{ = 0}}{\rm{.3}}\,\,{\rm{V}}\,\,{\rm{at}}\,\,{\rm{25^\circ C}}\). The equilibrium constant of the reaction is

330444 The equilibrium constant of the reaction:
\({{\text{A}}_{{\text{(s)}}}}{\text{ + 2B}}_{{\text{(aq)}}}^{\text{ + }} \rightleftharpoons {\text{A}}_{{\text{(aq)}}}^{{\text{2 + }}}{\text{2}}{{\text{B}}_{{\text{(s)}}}}{\text{;}}\,\,{\text{E}}_{{\text{cell}}}^{\text{o}}{\text{ = 0}}{\text{.0295}}\,\,{\text{V}}\)
\({\rm{is}}\,\,\left[ {\frac{{{\rm{2}}{\rm{.303}}\,\,{\rm{RT}}}}{{\rm{F}}}{\rm{ = 0}}{\rm{.059}}} \right]\)

330445 For a cell involving one electron \({\rm{E}}_{{\rm{cell}}}^{\rm{o}}{\rm{ = 0}}{\rm{.59 V}}\) at 298 K, the equilibrium constant for the cell reaction is:
\(\left[ {{\rm{Given}}\,\,{\rm{that}}\frac{{{\rm{2}}{\rm{.303RT}}}}{{\rm{F}}}{\rm{ = 0}}{\rm{.059 V}}\,\,{\rm{at}}\,\,{\rm{T = 298 K}}} \right]\)

330441 Match the columns.
Given: \(\left(\mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{\circ}=0.8, \mathrm{~K}_{\mathrm{sp}}(\mathrm{AgCl})=10^{-10}\right)\)

330442 The standard emf of a galvanic cell involving 2 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the redox reaction of the cell is

330443 For a cell involving two electron changes,
\({\rm{E}}_{{\rm{cell}}}^{\rm{o}}{\rm{ = 0}}{\rm{.3}}\,\,{\rm{V}}\,\,{\rm{at}}\,\,{\rm{25^\circ C}}\). The equilibrium constant of the reaction is

330444 The equilibrium constant of the reaction:
\({{\text{A}}_{{\text{(s)}}}}{\text{ + 2B}}_{{\text{(aq)}}}^{\text{ + }} \rightleftharpoons {\text{A}}_{{\text{(aq)}}}^{{\text{2 + }}}{\text{2}}{{\text{B}}_{{\text{(s)}}}}{\text{;}}\,\,{\text{E}}_{{\text{cell}}}^{\text{o}}{\text{ = 0}}{\text{.0295}}\,\,{\text{V}}\)
\({\rm{is}}\,\,\left[ {\frac{{{\rm{2}}{\rm{.303}}\,\,{\rm{RT}}}}{{\rm{F}}}{\rm{ = 0}}{\rm{.059}}} \right]\)

330445 For a cell involving one electron \({\rm{E}}_{{\rm{cell}}}^{\rm{o}}{\rm{ = 0}}{\rm{.59 V}}\) at 298 K, the equilibrium constant for the cell reaction is:
\(\left[ {{\rm{Given}}\,\,{\rm{that}}\frac{{{\rm{2}}{\rm{.303RT}}}}{{\rm{F}}}{\rm{ = 0}}{\rm{.059 V}}\,\,{\rm{at}}\,\,{\rm{T = 298 K}}} \right]\)

330441 Match the columns.
Given: \(\left(\mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{\circ}=0.8, \mathrm{~K}_{\mathrm{sp}}(\mathrm{AgCl})=10^{-10}\right)\)

330442 The standard emf of a galvanic cell involving 2 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the redox reaction of the cell is

330443 For a cell involving two electron changes,
\({\rm{E}}_{{\rm{cell}}}^{\rm{o}}{\rm{ = 0}}{\rm{.3}}\,\,{\rm{V}}\,\,{\rm{at}}\,\,{\rm{25^\circ C}}\). The equilibrium constant of the reaction is

330444 The equilibrium constant of the reaction:
\({{\text{A}}_{{\text{(s)}}}}{\text{ + 2B}}_{{\text{(aq)}}}^{\text{ + }} \rightleftharpoons {\text{A}}_{{\text{(aq)}}}^{{\text{2 + }}}{\text{2}}{{\text{B}}_{{\text{(s)}}}}{\text{;}}\,\,{\text{E}}_{{\text{cell}}}^{\text{o}}{\text{ = 0}}{\text{.0295}}\,\,{\text{V}}\)
\({\rm{is}}\,\,\left[ {\frac{{{\rm{2}}{\rm{.303}}\,\,{\rm{RT}}}}{{\rm{F}}}{\rm{ = 0}}{\rm{.059}}} \right]\)

330445 For a cell involving one electron \({\rm{E}}_{{\rm{cell}}}^{\rm{o}}{\rm{ = 0}}{\rm{.59 V}}\) at 298 K, the equilibrium constant for the cell reaction is:
\(\left[ {{\rm{Given}}\,\,{\rm{that}}\frac{{{\rm{2}}{\rm{.303RT}}}}{{\rm{F}}}{\rm{ = 0}}{\rm{.059 V}}\,\,{\rm{at}}\,\,{\rm{T = 298 K}}} \right]\)

330441 Match the columns.
Given: \(\left(\mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{\circ}=0.8, \mathrm{~K}_{\mathrm{sp}}(\mathrm{AgCl})=10^{-10}\right)\)

330442 The standard emf of a galvanic cell involving 2 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the redox reaction of the cell is

330443 For a cell involving two electron changes,
\({\rm{E}}_{{\rm{cell}}}^{\rm{o}}{\rm{ = 0}}{\rm{.3}}\,\,{\rm{V}}\,\,{\rm{at}}\,\,{\rm{25^\circ C}}\). The equilibrium constant of the reaction is

330444 The equilibrium constant of the reaction:
\({{\text{A}}_{{\text{(s)}}}}{\text{ + 2B}}_{{\text{(aq)}}}^{\text{ + }} \rightleftharpoons {\text{A}}_{{\text{(aq)}}}^{{\text{2 + }}}{\text{2}}{{\text{B}}_{{\text{(s)}}}}{\text{;}}\,\,{\text{E}}_{{\text{cell}}}^{\text{o}}{\text{ = 0}}{\text{.0295}}\,\,{\text{V}}\)
\({\rm{is}}\,\,\left[ {\frac{{{\rm{2}}{\rm{.303}}\,\,{\rm{RT}}}}{{\rm{F}}}{\rm{ = 0}}{\rm{.059}}} \right]\)

330445 For a cell involving one electron \({\rm{E}}_{{\rm{cell}}}^{\rm{o}}{\rm{ = 0}}{\rm{.59 V}}\) at 298 K, the equilibrium constant for the cell reaction is:
\(\left[ {{\rm{Given}}\,\,{\rm{that}}\frac{{{\rm{2}}{\rm{.303RT}}}}{{\rm{F}}}{\rm{ = 0}}{\rm{.059 V}}\,\,{\rm{at}}\,\,{\rm{T = 298 K}}} \right]\)

330441 Match the columns.
Given: \(\left(\mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{\circ}=0.8, \mathrm{~K}_{\mathrm{sp}}(\mathrm{AgCl})=10^{-10}\right)\)

330442 The standard emf of a galvanic cell involving 2 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the redox reaction of the cell is

330443 For a cell involving two electron changes,
\({\rm{E}}_{{\rm{cell}}}^{\rm{o}}{\rm{ = 0}}{\rm{.3}}\,\,{\rm{V}}\,\,{\rm{at}}\,\,{\rm{25^\circ C}}\). The equilibrium constant of the reaction is

330444 The equilibrium constant of the reaction:
\({{\text{A}}_{{\text{(s)}}}}{\text{ + 2B}}_{{\text{(aq)}}}^{\text{ + }} \rightleftharpoons {\text{A}}_{{\text{(aq)}}}^{{\text{2 + }}}{\text{2}}{{\text{B}}_{{\text{(s)}}}}{\text{;}}\,\,{\text{E}}_{{\text{cell}}}^{\text{o}}{\text{ = 0}}{\text{.0295}}\,\,{\text{V}}\)
\({\rm{is}}\,\,\left[ {\frac{{{\rm{2}}{\rm{.303}}\,\,{\rm{RT}}}}{{\rm{F}}}{\rm{ = 0}}{\rm{.059}}} \right]\)

330445 For a cell involving one electron \({\rm{E}}_{{\rm{cell}}}^{\rm{o}}{\rm{ = 0}}{\rm{.59 V}}\) at 298 K, the equilibrium constant for the cell reaction is:
\(\left[ {{\rm{Given}}\,\,{\rm{that}}\frac{{{\rm{2}}{\rm{.303RT}}}}{{\rm{F}}}{\rm{ = 0}}{\rm{.059 V}}\,\,{\rm{at}}\,\,{\rm{T = 298 K}}} \right]\)