The cell reaction of the galvanic cell, Cu(s) // Cu^(2+)(aq) // Hg^(2+) (aq) // Hg (l) is
Write the equation for rthe rate of the reaction 5 Br_((aq))^(-)+BrO_(3(aq))^(-)+6H_((aq))^(+)to 3Br _((aq))+3H_(2)O_((l))
Write the Nernst equation for the EMF of the cell Ni _((s))|Ni +_((aq))^(2+)||Ag_((aq))^(+)|Ag
Write the cell reaction taking plce in the cell CU_((s))|Cu_((aq))^(+2)||Ag _((aq))^(+) |Ag _((s))
The standard reduction potentials for two reactions are given below: AgCl(s) + e^(-) to Ag(s) + Cl^(-) , E^@ = 0.22 V Ag^(+)(aq) e^(-) +e^(-) to Ag(s) , E^@ = 0.80V The solubility product of AgCl under standard conditions of temperature (298 K) is given by
Using the standard electron potentials given in the Table 8.1, predict if the reaction between the following is feasible : (a) Fe^(3+) (aq) and I^(-) (aq) (b) Ag^(+)(aq) and Cu(s) (c) Fe^(3+) (aq) and Cu (s) (d) Ag(s) and Fe^(3+)(aq) (e) Br_(2) (aq) and Fe^(2+) (aq)
Identify the substance oxidised, reduced, oxidising agent and reducing agent for each of the following reactions : a) 2AgBr(s)+C_(6)H_(6)O_(2)(aq)to2Ag(s)+2HBr(aq)+C_(6)H_(4)O_(2)(aq) b) HCHO(l)+2[Ag(NH_(3))_(2))^(+)(aq)+3OH^(-)(aq)to2Ag(s)+HCOO^(-)(aq)+4NH_(3)(aq)+2H_(2)O(l) c) HCHO(l)+2Cu^(2+)(aq)+5OH^(-)(aq)toCu_(2)O(s)+HCOO^(-)(aq)+3H_(2)O(l) d) N_(2)H_(4)(l)+2H_(2)O_(2)(l)toN_(2)(g)+4H_(2)O(l) e) Pb(s)+PbO_(2)(s)+2H_(2)SO_(4)(aq)to2PbSO_(4)(s)+2H_(2)O(l)
Calculate the standard cell potentials of galvanic cell in which the following reactions take place. (i) 2Cr(s) + 3Cd^(2+)(aq) to 2Cr^(3+) (aq) + 3Cd (ii) Fe^(2+)(aq) + Ag^(+)(aq) to Fe^(3+)(aq) + Ag(s) Calculate the ΔrG and equilibrium constant of the reactions.
