Electrochemistry · Chemistry · JEE Advanced

An aqueous solution of hydrazine $\left(\mathrm{N}_2 \mathrm{H}_4\right)$ is electrochemically oxidized by $\mathrm{O}_2$, thereby releasing chemical ...

Some standard electrode potentials at 298 K are given below :Pb2+ /Pb = $$- $$0.13 VNi2+ /Ni = $$-$$ 0.24 VCd2+ /Cd = $$-$$ 0.40 VFe2+ /Fe = $$-$$ 0.4...

In a galvanic cell, the salt bridge

For the reduction of NO$$_3^ - $$ ion in an aqueous solution, E$$^0$$ is + 0.96 V. Values of E$$^0$$ for some metal ions are given below: $$\matrix{ ...

In a conductometric titration, small volume of titrant of higher concentration is added stepwise to a larger volume of titrate of much lower concentra...

Plotting $1 / \Lambda_{\mathrm{m}}$ against $\mathrm{c} \Lambda_{\mathrm{m}}$ for aqueous solutions of a monobasic weak acid $(\mathrm{HX})$ resulted ...

Molar conductivity ($$\Lambda $$m) of aqueous solution of sodium stearate, which behaves as a strong electrolyte, is recorded at varying concentration...

For the following cell, $$Zn\left( s \right)\left| {ZnS{O_4}\left( {aq} \right)} \right|\left| {CuS{O_4}\left( {aq} \right)} \right|Cu\left( s \right)...

For the following electrochemical cell at 298 K Pt(s) | H2 (g, 1 bar) | H+ (aq, 1 M) || M4+ (aq), M2+ (aq) | Pt (s) Ecell = 0.092 V when $${{\left[ {...

An aqueous solution of X is added slowly to an aqueous solution of Y as shown in List – I. The variation in conductivity of these reactions in List – ...

The standard reduction potential data at 25oC is given below: Eo (Fe3+ , Fe2+) = +0.77V; Eo (Fe2+ , Fe) = -0.44V; Eo (Cu2+ , Cu) = +0.34V; Eo (Cu+ ...

The electrochemical cell shown below is a concentration cell. M | M2+ (saturated solution of a sparingly soluble salt, MX2) || M2+ (0.001 mol dm–3) | ...

The electrochemical cell shown below is a concentration cell. M | M2+ (saturated solution of a sparingly soluble salt, MX2) || M2+ (0.001 mol dm–3) | ...

AgNO3(aq.) was added to an aqueous KCl solution gradually and the conductivity of the solution was measured. The plot of conductance ($$\Lambda $$) ve...

Consider the following cell reaction: 2Fe(s) + O2(g) + 4H+(aq) $$\to$$ 2Fe2+ (aq) + 2H2O (l); Eo = 1.67 V At [Fe2+] = 10-3 M, P(O2) = 0.1 atm and pH =...

The concentration of potassium ions inside a biological cell is at least twenty times higher than the outside. The resulting potential difference acro...

The concentration of potassium ions inside a biological cell is at least twenty times higher than the outside. The resulting potential difference acro...

Electrolysis of dilute aqueous NaCl solution was carried out by passing 10 milli ampere current. The time required to liberate 0.01 mol of H$$_2$$ gas...

Consider the strong electrolytes $Z_{m} X_{n}, U_{m} Y_{p}$ and $V_{m} X_{n}$. Limiting molar conductivity ( $\Lambda^{0}$ ) of $\mathrm{U}_{\mathrm{m...

The reduction potential $\left(E^{0}\right.$, in $\left.\mathrm{V}\right)$ of $\mathrm{MnO}_{4}^{-}(\mathrm{aq}) / \mathrm{Mn}(\mathrm{s})$ is _______...

At 298 K, the limiting molar conductivity of a weak monobasic acid is 4 $$\times$$ 102 S cm2 mol$$-$$1. At 298 K, for an aqueous solution of the acid ...

At 298 K, the limiting molar conductivity of a weak monobasic acid is 4 $$\times$$ 102 S cm2 mol$$-$$1. At 298 K, for an aqueous solution of the acid ...

Consider a 70% efficient hydrogen-oxygen fuel cell working under standard conditions at 1 bar and 298 K. Its cell reaction is $${H_2}(g) + {1 \over 2}...

Consider an electrochemical cell : $$A\left( s \right)\left| {{A^{n + }}\left( {aq,2M} \right)} \right|{B^{2n + }}\left( {aq,1M} \right)\left| {B\lef...

For the electrochemical cell, $$\left. {Mg\left( s \right)} \right|M{g^{2 + }}\left( {aq,1\,M} \right)\left\| {C{u^{2 + }}} \right.\left( {aq,1M} \ri...

The conductance of a $$0.0015$$ $$M$$ aqueous solution of a weak monobasic acid was determined by using a conductivity cell consisting of platinized $...

The molar conductivity of a solution of a weak acid HX (0.01 M) is 10 times smaller than the molar conductivity of a solution of a weak acid HY (0.10 ...

All the energy released from the reaction $$X \to Y, \Delta _tG^o $$ = -193 kJ mol-1 is used for oxidizing M+ as M+ $$\to$$ M3+ + 2e-, Eo = -0.25 V U...

We have taken a saturated solution of AgBr. Ksp of AgBr is 12 $$\times$$ 10-14. If 10-7 mole of AgNO3 are added to 1 litre of this solution find condu...

(a). For the reaction Ag+ (aq) + Cl- (aq) $$\leftrightharpoons$$ AgCl (s) Given: .tg {border-collapse:collapse;border-spacing:0;} .tg td{font-famil...

Find the equilibrium constant for the reaction, In2+ + Cu2+ $$\to$$ In3+ + Cu+ at 298 K given $$E_{C{u^{2 + }}/C{u^ + }}^o$$ = 0.15 V; $$E_{l{n^{2 + }...

Two students use the same stock solution of ZnSO4 and solution of CuSO4. The emf of one cell is 0.03 V higher than other. The conc. of CuSO4 in the ce...

The standard potential of the following cell is 0.23V at 15oC and 0.21 V at 35oC. Pt | H2 (g) | HCl (aq) | AgCl (s) | Ag (s) (i) Write the cell reacti...

The following electrochemical cell has been set up. Pt(1) | Fe3+, Fe2+ (a = 1) | Ce4+, Ce3+ (a=1) | Pt(2) Eo (Fe3+, Fe2+) = 0.77 V; Eo (Ce4+, Ce3+) = ...

Copper sulphate solution (250 mL) was electrolysed using platinum anode and a copper cathode. A constant current of 2mA was passed for 16 minutes. It ...

A cell, Ag | Ag+ || Cu2+ | Cu, initially contains 1 M Ag+ and 1 M Cu2+ ions. Calculate the change in the cell potential after the passage of 9.65 A cu...

Calculate the equilibrium constant for the reaction: 2Fe3+ + 3I- $$\leftrightharpoons$$ 2Fe2+ + $$I_3^-$$. The standard reduction potentials in acidic...

Find the solubility product of a saturated solution of Ag2CrO4 in water at 298 K if the emf of the cell Ag|Ag+ (satd. Ag2CrO4 soln.) || Ag+ (0.1 M) | ...

How many grams of silver could be plated out on a serving tray by electrolysis of a solution containing silver in +1 oxidation state for a period of 8...

Calculate the equilibrium constant for the reaction Fe2+ + Ce4+ $$\leftrightharpoons$$ Fe3+ + Ce3+ (given $$E_{C{e^{4 + }}/C{e^{3 + }}}^o$$ = 1.44 V; ...

The standard reduction potential for Cu2+|Cu is +0.34 V. Calculate the reduction potential at pH = 14 for the above couple. Ksp of Cu(OH)2 is 1.0 $$\t...

An excess of liquid mercury is added to an acidified solution of 1.0 $$\times$$ 10-3 M Fe3+. It is found that 5% of Fe3+ remains at equilibrium at 25o...

The standard reduction potential of the Ag+/Ag electrode at 298 K is 0.799V. Given that for AgI, Ksp = 8.7 $$\times$$ 10-17, evaluate the potential of...

The Edison storage cells is represented as Fe(s) | FeO(s) | KOH (aq) | Ni2O3(s) | Ni(s) The half-cell reactions are: Ni2O3 + H2O (l) + 2e- $$\leftrigh...

The standard reduction potential for the half-cell $$NO_3^-$$ + 2H+ (aq) + e $$\to$$ NO2 (g) + H2O is 0.78 V (i) Calculate the reduction potential in ...

Chromium metal can be plated out from an acidic solution containing CrO3 according to the following equation CrO3 (aq) + 6H+ (aq) + 6e- $$\to$$ Cr(s)...

An aqueous solution of NaCl on electrolysis gives H2(g), Cl2(g) and NaOH according to the reaction: 2Cl- (aq) + 2H2O = 2OH- (aq) + H2 (g) + Cl2 (g) A ...

For the galvanic cell Ag | AgCl(s), KCl (0.2M) || KBr (0.001M), AgBr(s) | Ag Calculate the EMF generated and assign correct polarity to each electrode...

The current of 1.70 A is passed through 300.0 ml of 0.160 M solution of a ZnSO4 for 230 sec. with a current efficiency of 90%. Find out the molarity o...

Zinc granules are added in excess to a 500 ml. of 1.0 M nickel nitrate solution at 25oC until the equilibrium is reached. If the standard reduction po...

(i) What is the weight of sodium bromate and molarity pf solution necessary to prepare 85.5 ml of 0.672 B solution when the half-cell reaction is $$Br...