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 .

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

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

Write the Nernst equation and emf of the following cells at 298 K: Mg(s)|Mg^(2+)(0.001M) || Cu^(2+)(0.0001 M)| Cu(s)

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 .

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

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

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

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.

The following chemical Feaction is occurring in an electrochemical cell. Mg(s) + 2 Ag^(+) (0.0001 M)rarr Mg^(2+) (0.10 M) + 2 Ag (s) The E^@ electrode values are Mg^(2+)//Mg = -2.36 V Ag^(+)//Ag = 0.81 V For this cell, calculate/write : Cell potential E_(cell) .