The standard reduction potentials of Cu²⁺/Cu and Cu²⁺/Cu⁺ are 0.337 and 0.153V respectively. The standard electrode potential of Cu⁺/Cu half cell is:

When a lead storage battery is discharged, then:

Metals have conductivity of the order of (ohm^-1 m^-1):-

An electrochemical cell is shown below Pt, H₂(1 atm)| HCI (0.1 M)CH₃COOH (0.1 M)|

H₂(1 atm), Pt The EMF of the cell will not be zero, because

1. EMF depends on molarities of acids used

Saturated solution of KNO₃ is used to make 'salt-bridge' because:

A current is passed through two voltameters connected in series. The first voltmeter connected in series. The first voltmeter contains XSO₄(aq) while the second voltmeter contains Y₂SO₄(aq). The relative  atomic masses of X and Y are in the ratio of 2:1. The ration of the mass of X liberated to the mass of Y liberated is: 

The mass of silver(eq. mass = 108) displaced by that quantity of current which displaced 5600 mL of hydrogen at STP is:

A silver cup is plated with silver by passing 965 coulomb of electricity. The amount of Ag deposited is:

Which is the correct representation for Nernst equation ?

When a copper wire is immersed in a solution of AgNO₃, the colour of solution becomes blue because copper:

The specific conductance of a 0.1N KCl solution at 23$°\mathrm{C}$ is 0.012 ${\mathrm{\Omega }}^{-1}{\mathrm{cm}}^{-1}$. The resistance of cell containing the solution at the same temperature was found to be 55 $\mathrm{\Omega }$. The cell constant will be 

Given below are the half-cell reactions,

Mn²⁺ + 2e^-  $\to \; Mn; \; \; \; \; \; \; E0\; =\; -1.18V$

$$ \to \; 2Mn2+; \; E0\; =\; +1.51V$$

$$ E0 for\; 3\; Mn2+ \to \; 2\; Mn+3 \; +$$Mn will be:

E⁰ for Fe²⁺ + 2e → Fe is -0.44 volt and E⁰ for Zn²⁺ + 2e→ Zn is -0.76 volt, thus:

The voltage of the given below cell is increased by : 

$$\begin{gathered} \mathrm{Cell}: \mathrm{Sn}\left(\mathrm{s}\right) + 2{\mathrm{Ag}}^{+}\left(\mathrm{aq}\right) \stackrel{ }{\to } \\ {\mathrm{Sn}}^{2+}\left(\mathrm{aq}\right) + 2\mathrm{Ag}\left(\mathrm{s}\right) \end{gathered}$$

A 5A current is passed through a solution of copper sulphate for 40 min. The amount of copper deposited at the cathode is 

$E_{\raisebox{1ex}{${\mathrm{Fe}}^{2+}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Fe}$}\right.}^{\circ } = -0.441 \mathrm{V} and E_{\raisebox{1ex}{${\mathrm{Fe}}^{3+}$}\!\left/ \!\raisebox{-1ex}{${\mathrm{Fe}}^{2+}$}\right.}^{\circ } =0.771 \mathrm{V}$, the standard emf of the reaction

$\mathrm{Fe} + 2{\mathrm{Fe}}^{3+} \stackrel{ }{\to }3{\mathrm{Fe}}^{2+}$will be

Standard electrode potential for Sn⁴⁺ / Sn²⁺ couple is +0.15 V and that for the Cr³⁺/Cr couple is -0.74. These two couples in their standard state are connected to make a cell. The cell potential will be : 

If an iron rod is dipped in CuSO₄ solution, then:

Without losing it's concentration ZnCl₂ solution cannot be kept in contact with :

Al₂O₃ is reduced by electrolysis at low potentials and high currents. If 4.0 x 10⁴ A of current is passed through molten Al₂O₃ for 6 h, what mass of aluminium is produced? (Assume 100% current efficiency, atomic mass of Al = 27g mol^-1)

The standard reduction potential at 290 K for the following half reactions are,

(i) Zn²⁺ + 2e— → Zn(s);      E° = -0.762 V

(ii) Cr³⁺ + 3e → Cr(s);          E° = -0.740 V

(iii) 2H⁺ + 2e → H₂(g); ·      E° = +0.000 V

(iv) Fe³⁺ + e → Fe²⁺;         E° = +0.77V

Which is the strongest reducing agent?

The ratio of masses of hydrogen and magnesium deposited by the same amount of electricity from H₂SO₄ and MgSO₄ in aqueous solution are:

The molar conductances of Ba²⁺ and Cl^- 127 and 76Ω^-1 cm^-1 mol^-1 respectively at infinite dilution. The equivalent conductance of BaCl₂ at infinite dilution will be

A depolariser used in dry cell batteries is: 

The reaction taking place  at anode when an aqueous solution of CuSO₄ is electrolysed using inert Pt electrode:

An increase in equivalent conductance of a strong electrolyte with dilution is mainly due to

For the cell, Ti|Ti⁺(0.001M)||Cu²⁺(0.1M)|Cu,E_cell at 25$°$C is 0.83 V. E_cell can be increased:

The atomic mass of Al is 27. When a current of 5 faraday is passed through a solution of Al³⁺ ions, the mass of Al deposited is:

Which graph correctly correlates E_cell as a function of concentrations for the cell (for different values of M and M') ?

$$\begin{gathered} \mathrm{Zn}\left(\mathrm{s}\right) + {\mathrm{Cu}}^{2+}\left(M\right) \stackrel{ }{\to }{\mathrm{Zn}}^{2+}(M\text{'}) + \mathrm{Cu}\left(\mathrm{s}\right); \\ E_{\mathrm{cell}}^{\circ } = 1.10 \mathrm{V} \\ X-\mathrm{axis} : {\log }_{10}\frac{\left[{\mathrm{Zn}}^{2+}\right]}{\left[{\mathrm{Cu}}^{2+}\right]}, Y-\mathrm{axis} : E_{\mathrm{cell}} \end{gathered}$$

The most convenient method to protect the bottom of the ship made of iron is