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the E(cell) and triangleG for the galvan...

the `E_(cell)` and `triangleG` for the galvanic cell `Cu(s)//Cu^(2+) (0.130M)||Ag^(+)(1.00times10^(-4)M)|Ag(s)` given that `E°(Cu^(2+)//Cu)=0.34V` and `E °(Ag^+//Ag)=0.80V`

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Write Nernst equation and calculate the e.m.f. of the following cell at 298 K: Cu(s)|Cu^(2+)(0.130M)||Ag^(+)(1.0xx10^(-4)M)|Ag(s) Given that: E_(Cu^(2+)//Cu)^(@)=+0.34V and E_(Ag^(+)//Ag)^(@)=+0.80V (log 0.130=-1.1139).

Derive Nernst equation for the following cell: Cu|Cu^(2+)(0.1M)||Ag^(+)(0*1M)|Ag

Calculate the e.m.f. of the following cell at 298 K, Mg|Mg^(2+)(0.130M)||Ag^(+)(1.0xx10^(-4)M)|Ag

Write each half cell reaction of the following electrochemical cell: Cu(s)|Cu^(2+)(1M)||Ag^(+)(1M)|Ag(s)

Write Nernst equation and calculate e.m.f. of the following cell at 298 k. Mg(s)|Mg^(2+)(0.130M)||Ag^+(0.0001M)|Ag(s) Given E^o(Mg^(2+)//Mg)=-2.37 V E^o(Ag^(+)//Ag)=0.80 V (log 1.3=0.1130)

Write the Nernst equation and calculate e.m.f of following cell at 298K. Mg(s)|Mg^(2+)(0.130M)||Ag^(+)(0.0001M)|Ag(s) Given E_(Mg^(2+)//Mg)^(@)=-2.37V,E_(Ag^(+)//Ag)^(@)=0.80V . (log 1.3=0.1130)

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