Electrochemistry

ABC26PH0398 · For the following reaction 2MnO4^- + 5H2C2O4 + 6H^+ → 2Mn2+ + 8H2O + 10CO2; E0(MnO4^-/Mn2+) = +1.51 V and E0(CO2/H2C2O4) = -0.49 V. At 298… · 2005-2021

ABC26PH0399 · A sparingly soluble electrolyte M2X ionizes as M2X ⇌ 2M^+ + X2-. The solubility product (Ksp), molal solubility (S) and molal activity… · 2005-2021 self-practice

ABC26PH0704 · The mean ionic activity coefficient for a 0.01 M aqueous solution of Ca3(PO4)2 is ____ (Round off to three decimal places) (Given : log 10… · 2001-2022 self-practice

ABC26PH0705 · For the reaction, CuSO4(aq) + Zn(s) → ZnSO4(aq) + Cu(s), the value of Delta G° (in kJ mol-1) is ____ (Round off to the nearest integer)… · 2001-2022 self-practice

ABC26PH0985 · In a potentiometric titration, the end point is obtained by observing · DEC 2013

ABC26PH0401 · The value of log e(KSP) for Fe(OH)3 at 298 K is · 2005-2021

ABC26PH0986 · Electrolysis of an aqueous solution of 1.0 M NaOH results in · DEC 2013

ABC26PH0402 · A platinum electrode is immersed in a solution containing 0.1 M Fe2+ and 0.1 M Fe3+. Its potential is found to be 0.77V against SHE. Under… · 2005-2021 self-practice

ABC26PH0987 · The cell voltage of Daniel cell [Zn |ZnSO4(aq) | CuSO4(aq) | Cu] is 1.07 V. If reduced potential of Cu2+ Cu is 0.34 V, the reduction… · DEC 2013

ABC26PH0403 · Given the E0 values for the following reaction sequence, Mn6+ 1.28 V Mn5+ 2.9 V Mn4+ 0.96 Mn3+ 1.5 V Mn2+ the computed value of E0 for Mn6+… · 2005-2021 self-practice

ABC26PH0404 · The expression for the equilibirum constant (Keq) for the enzyme catalyzed reaction given below, is E+S k2k1⇌ ES k4k3⇌ P+E · 2005-2021

ABC26PH0405 · The solubility product of AgBr(s) is 5 × 10-13 at 298 K. If the standard reduction potential of the half-cell, E0Ag|AgBr(s)|Br^- is 0.07 V… · 2005-2021 self-practice

ABC26PH0060 · The temperature-dependence of an electrochemical cell potential is · JUNE 2015

ABC26PH0412 · The temperature derivative of electrochemical potential E at constant pressure, ((∂ E)/(∂ T))P is given by · 2005-2021 self-practice

ABC26PH0996 · The temperature-dependence of an electrochemical cell potential is · JUNE 2015

ABC26PH0063 · Given that Eo(Cl2/Cl^-) = 1.35 V and Ksp(AgCl) = 10-10 at 25°C, Eo corresponding to the electrode reaction 1/2Cl2(g) + Ag^+(Soln.) + e^- →… · DEC 2015

ABC26PH0416 · The activity of ' m ' molal CuSO4 solution can be expressed in terms of its mean activity coefficient (gamma ±)as: · 2005-2021 self-practice

ABC26PH0065 · In a potentiometric titration, the end point is characterised by · JUNE 2016 self-practice

ABC26PH1002 · In a potentiometric titration, the end point is characterised by · JUNE 2016

ABC26PH0419 · In an electrochemical cell, Ag^+ ions in AgNO3 are reduced to Ag metal at the cathode and Cu is oxidized to Cu2+ at the anode. A current of… · 2005-2021 self-practice

ABC26PH0067 · Given (i) Zn + 4NH3 → Zn(NH3)42+ + 2e, Eo = 1.03 V (ii) Zn → Zn+2 + 2e, E0 = 0.763 V the formation constant of the complex Zn(NH3)42+ is… · DEC 2016

ABC26PH1008 · Given : (i) Zn + 4NH3 → Zn(NH3)42+ + 2e, E0 = 1.03 V (ii) Zn → Zn+2 + 2e, E° = 0.763 V the formation of the complex Zn(NH3)42+ is… · DEC 2016

ABC26PH1010 · The electrochemical cell potential (E), after the reactants and products reach equilibrium, is (E0 is the standard cell potential and n is… · JUNE 2017

ABC26PH1012 · The standard cell potential for the reaction Zn(s) + Cu2+(aq) ⇔ Zn2+(aq) + Cu(s) is +1.10 V. The Gibbs free energy change during the… · JUNE 2017

ABC26PH0069 · The standard cell potential of cell, Pt | H2(g) | HBr(aq) | AgBr(s) | Ag(s), was measured over a range of temperatures, and the data was… · JUNE 2017

ABC26PH1014 · The standard cell potential of cell, Pt | H2(g) | HBr(aq) | AgBr(s) | Ag(s), was measured over a range of temperatures, and the data was… · JUNE 2017

ABC26PH0070 · The correct statement among the following is · DEC 2018

ABC26PH1015 · The correct statement among the following is · DEC 2017

ABC26PH0071 · The standard free energy of the reaction AgBr(s) → Ag^+(aq) + Br^-(aq) Is closest to. [Eo(AgBr/Ag, Br^-) = 0.07 V; Eo(Ag/Ag^+) = 0.80 V; F… · DEC 2018

ABC26PH1016 · The standard free energy of the reaction AgBr(s) → Ag+(aq) + Br-(aq) Is closest to. [E°(AgBr/Ag,Br-) = 0.07 V; E°(Ag/Ag+) = 0.80 V; F =… · DEC 2017

ABC26PH0072 · Conductivities of water and a saturated solution of a sparingly soluble salt AB2 are 7 and 21 mu S m-1, respectively. Given, lambda o_A2+ =… · DEC 2018

ABC26PH1017 · Conductivities of water and a saturated solution of a sparingly soluble salt AB2 are 7 and 21 mu S m-1, respectively. Given lambda… · DEC 2017

ABC26PH0073 · The equilibrium constant of the following reaction: Sn(s) + Sn4+(aq) ⇌ 2Sn2+(aq) At 300 K is closest to, (Given, Eo_Sn4+/Sn2+ = 0.15 V and… · DEC 2018

ABC26PH1018 · The equilibrium constant of the following reaction: Sn(s)+Sn4+(aq) ⇔ 2 Sn2+(aq) At 300 K is closest to, (Given : E_Sn4+ / Sn2+o=0.15 V and… · JUNE 2018

ABC26PH1019 · The mobility of a divalent cation in water is 8×10-8m2V-1s-1. The effective radius of the ion is (viscosity of water =1cP; e=1.6×10-19C) · JUNE 2019

ABC26PH1020 · If the over potential of an electrolysis process is increased from 0.5V to 0.6V, then the ratio of current densities (ln J0.6/J0.5) of the… · JUNE 2019

ABC26PH0075 · For the electrochemical cell Ag|AgCl|MCl(0.01 M)|MCl(0.02 M)|AgCl|Ag, the junction potential is the highest when M^+ is · DEC 2019

ABC26PH1023 · For the electrochemical cell Ag | AgCl | MCl (0.01 M) | MCl (0.02 M) | AgCl | Ag, the junction potential is the highest when M^+ is · DEC 2019

ABC26PH1025 · The E0(M^+/M) of the cell, SHE | MX | M can be obtained from the plot of (Ecell is the cell potential and m is molality of ideal dilute… · DEC 2019

ABC26PH1027 · For the cell Cd | CdCl2 || AgCl | Ag; E°cell = 0.675 V and dE°cell/dT = -6.5 × 10-4 V K-1 at 27°C. The Delta H (kJ mol-1) value for the… · JUNE 2021

ABC26PH0074 · If the overpotential of an electrolysis process is increased from 0.5 V to 0.6 V, then the ratio of current densities (ln J0.6/J0.5) of the… · JUNE 2019 self-practice

ABC26PH0384 · If standard emf of the cell, Cu | Cu2+(aq) | [Cu(NH3)4]2+, aq.NH3 | Cu is 0.35, then stability constant of the formation cupric amine… · 2005-2021 self-practice

ABC26PH0689 · The statement that is correct for both electrochemical (galvanic) cells and electrolytic cell is : · 2001-2022

ABC26PH0690 · The standard potential of a Daniel cell is +1.10 V and the equilibrium constant for the cell reaction is 1.5 × 1037. It can be concluded… · 2001-2022

ABC26PH0387 · Given the standard potential for the following half-cell reaction at 298 K Cu+(aq)+e- → Cu(s) E0=0.52 V Cu2+(aq)+e- → Cu+(aq) E0=0.16 V… · 2005-2021

ABC26PH0972 · For a potentiometric titration, in the curve of emf (E) vs volume (V) of the titrant added, the equivalence point is indicated by · DEC 2011

ABC26PH0973 · The standard electrode potentials (E°) of Fe3+/Fe2+ and Fe2+/Fe electrodes are + 0.77V and -0.44 V respectively at 300 K. The E° of Fe3+/Fe… · DEC 2011

ABC26PH0394 · The standard reduction potentials at 298 K for single electrodes are given below: From this we can infer that · 2005-2021 self-practice

ABC26PH0699 · An electrochemical cell consists of two half-cell reactions AgCl(s) + e^- → Ag(s) + Cl^-(aq); Cu(s) → Cu2+(aq) + 2e^- The mass of copper… · 2001-2022

ABC26PH0700 · For a cell reaction, Pb(s) + Hg2Cl2(s) → PbCl2(s) + 2Hg(l), ((∂ Eo)/(∂ T))P is 1.45 × 10-4 V K-1. The entropy change (in J mol-1 K-1) for… · 2001-2022 self-practice