The `E^(@)` at `25^(@)` for the following reaction at the indicated concentration is 1.50 V. Calculate the `DeltaG` in kJ at `25^(@)` C:
`Cr(s)+3Ag^(+)(aq,0.1M)`
`rarrAg(s)+Cr^(3+)(aq,0.1M)`

The E^(@) at 25^(@) C for the following reaction at the indicated concentrations is 1.50 V. Calculate the DeltaG in kJ // mol 25^(@) C :

The E^(@) at 25^(@) C for the following reaction at the indicated concentrations is 1.50 V. Calculate the DeltaG in kJ // mol 25^(@) C :

The E^(@) at 25^(@)C for the following reaction at the indicated concentrations is 1.50 V . Calculate the DeltaG in kJ at 25^(@)C , Cr(s) + 3Ag^(+) (aq. 0.1 M)to Ag(s) + Cr^(3+) (aq. 0.1 M)

The measured voltage for the reaction with the indicated concentration is 1.50 V. Calculate E^(@) . Cr(s)+3Ag^(+)(aq,0.10M)to3Ag(s)+Cr^(3+)(aq,0.30 M)

The measured voltage for the reaction with the indicated concentration is 1.50 V. Calculate E^(@) . Cr(s)+3Ag^(+)(aq,0.10M)to3Ag(s)+Cr^(3+)(aq,0.30 M)

Determine DeltaG^(@) and the value of the equilibrium constant for the following reaction occurring in an electrochemical cell at 25^(@)C . Cu(s)+2Ag^(+)(aq)rarr Cu^(2+)(aq)+2Ag(s) Given that, E_(Cu^(2+)|Cu)^(@)=0.34V and E_(Ag^(+)|Ag)^(@)=0.80V

The standard electrode potential for the following reaction is +1.33V . What is the potential at pH =2.0 ? Cr_(2)O_(7)^(2-)(aq,1M)+14H^(+)(aq)+6e^(-) rarr 2Cr^(3+)(aq. 1M)+7H_(2)O(l)

What is the approximate value of the equilibrium constant, K_(eq) , at 25^(@) C for the reaction, 3Ag^(+)(aq) + Cr(s) rightarrow Cr^(3+)(aq) + 3Ag(s)

Determine DeltaG^@ and the value of the equlibrium constant for the following reaction occurring in an electrochemical cell at 25^@C . Cu (s) + 2Ag^+ (aq) rarr Cu^(2+)(aq)+2Ag(s) Given that E_(Cu^(2+)//Cu)^@=0.34 V and E_(Ag^+//Ag)^@ =0.80V