calculate the e.m.f of the cell in which the following reaction takes place:
`Ni(s) +2Ag^(+) (0.002M)rarrNi^(2+) (0.160 M)+2Ag(s)`
Given that `E_(cell)^o=1.05V`

Calculate the emf of the cell in which the following reaction takes place: Ni(s) + 2Ag^+ (0.002 M) Ni^(2+) (0.160 M) + 2Ag(s) Given that E^V_(cell) = 1.05 V

Represent the cell in which the following reaction takes place Mg(s) + 2Ag^+(0.0001M) to Mg^(2+)(0.130M) + 2Ag(s) Calculate its E_(cell) if E_(cell) = 3.17 V.

Represent the cell in which the following reaction takes place: Mg(s)+Cu^(2+)(0.0001M) to Mg^(2+)(0.1M)+Cu(s) . Calculate its E, if E^(@) is 2.71V .

Caculate the E_(cell)^@ for the following reaction at 298K: 2Cr(s)+3Fe^(2+)(0.01M)rarr2Cr^(3+)(0.01M)+3Fe(s) Given E_(cell)=0.261V .

Which of the following will increase the voltage of the cell Sn(s)+2Ag^(+)(aq)rarrSn^(2+)(aq)+2Ag(s)

For the reaction : Ni(s)+2Ag^(+)(1M)rarrNi^(+2)(1M)+2Ag(s) . Which species get reduced?

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).

Write the Nernst equation and calculate E.M.F of the following reaction at 298 K Mg // Mg^(2+) (0.1 M)"//" Cu^(2+) (0.01 M) // Cu (s) given E_("cell")^0 = 2.71V,F=96500 C//mol

In the button cell widely used for watches and other devices, the following reaction takes place: Zn(s)+Ag_2O(s)+H_2O(l)rarrZn^(2+)(aq)+2Ag(s)+2OH^(-)(aq) Determine the value of K_c for the above reaction using the following data? AgO_2(s)+H_2O(l)+2barerarr2Ag(s)+2Oh^(-)(aq) ( E^@=0.344V ) Zn^(2+)(aq)+2barerarrZn(s) ( E^@=-0.76V )

In the button cells widely used in watches and other devices the following reaction takes place: Zn(s) + Ag20(s) + H2O(l) Zn2+(aq) + 2Ag(s) + 20H“(aq) Determine rG and E for the reaction.