Chemistry
Electrochemistry
Previous Years Questions

Numerical

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\left...
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 $${{\left[ {... An aqueous solution of X is added slowly to an aqueous solution of Y as shown in List – I. The variation in conductivity of these reactions in List – ... The standard reduction potential data at 25oC is given below: Eo (Fe3+ , Fe2+) = +0.77V; Eo (Fe2+ , Fe) = -0.44V; Eo (Cu2+ , Cu) = +0.34V; Eo (Cu+ ... The electrochemical cell shown below is a concentration cell. M | M2+ (saturated solution of a sparingly soluble salt, MX2) || M2+ (0.001 mol dm–3) | ... The electrochemical cell shown below is a concentration cell. M | M2+ (saturated solution of a sparingly soluble salt, MX2) || M2+ (0.001 mol dm–3) | ... Consider the following cell reaction: 2Fe(s) + O2(g) + 4H+(aq)$$\to$$2Fe2+ (aq) + 2H2O (l); Eo = 1.67 V At [Fe2+] = 10-3 M, P(O2) = 0.1 atm and pH =... The concentration of potassium ions inside a biological cell is at least twenty times higher than the outside. The resulting potential difference acro... The concentration of potassium ions inside a biological cell is at least twenty times higher than the outside. The resulting potential difference acro... Subjective We have taken a saturated solution of AgBr. Ksp of AgBr is 12$$\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...
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 ...
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+) = ...
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)...
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...
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 ...
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...
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...
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