If the molar conductance values of Ca²⁺ and Cl^- at infinite dilution are respectively 118.88 X 10^-4 m² $\mathrm{\Omega }$ho mol^-1 and 77.33 X 10^-4m² $\mathrm{\Omega }$ho mol^-1 then that of CaCl₂ is ( in m² $\mathrm{\Omega }$ho mol^-1): 

• 118.88 X 10^-4

• 154.66  X 10^-4

• 273.54  X 10^-4

• 196.21 X 10^-4

402.

The ionic conductance of Ba²⁺ and Cl^- are respectively 127 and 76 ohm^-1 cm² at infinite dilution. The equivalent conductance (in ohm^-1cm²) of BaCl₂ at infinite dilution will be

• 139.5

• 203

• 279

• 101.5

The reduction electrode potential, E of 0.1 M solution of M⁺ ions (E_RP = -2.36 V) is

• -4.82 V

• -2.41 V

• +2.41 V

• None of these

The amount of silver deposited on passing 2 F of electricity through aqueous solution of AgNO₃

• 54g

• 108g

• 216g

• 324g

EMF of hydrogen electrode in term of pH is (at 1 atm pressure).

• ${\mathrm{E}}_{{\mathrm{H}}_2}=\frac{\mathrm{RT}}{\mathrm{F}}\times \mathrm{pH}$

• ${\mathrm{E}}_{{\mathrm{H}}_2}=\frac{\mathrm{RT}}{\mathrm{F}}·\frac{1}{\mathrm{pH}}$

• ${\mathrm{E}}_{{\mathrm{H}}_2}=\frac{2.303 \mathrm{RT}}{\mathrm{F}}\mathrm{pH}$

• ${\mathrm{E}}_{{\mathrm{H}}_2}=- 0.591 \mathrm{pH}$

For the cell reaction, 

2Ce⁴⁺ + Co → 2Ce³⁺ + Co³⁺; E${}_{\mathrm{cell}}^{°}$ is 1.89 V. If ${\mathrm{E}}_{{\mathrm{Co}}^{2+}/ \mathrm{Co}}$ is -0.28V, what is the value of ${\mathrm{E}}_{{\mathrm{Ce}}^{4+} / {\mathrm{Ce}}^{3+}}^{°}$?

• 0.28 V

• 1.61 V

• 2.17 V

• 5.29 V

The equivalent conductance of silver nitrate solution at 250°C for an infinite dilution was found to be 133.3 $\mathrm{\Omega }$^-1 cm² equiv^-1. The transport number of Ag⁺ ions in very dilute solution of AgNO₃ is 0.464. Equivalent conductances of Ag⁺ and NO₃^- (in Ω^-1 cm² equiv^-1) at infinite dilution are respectively.

• 195.2; 133.3

• 61.9; 71.4

• 71.4; 61.9

• 133.3; 195.2

The standard reduction potential for Mg²⁺ /Mg is - 2.37 V and for Cu²⁺ /Cu is 0.337. The E${}_{\mathrm{cell}}^{°}$ for the following reaction is

Mg + Cu²⁺ → Mg²⁺ + Cu

• +2.03 V

• -2.03 V

• -2.7 V

• +2.7 V

Cu⁺ (aq) is unstable in solution and undergoes simultaneous oxidation and reduction, according to the reaction

                    $2{\mathrm{Cu}}^{+}\left(\mathrm{aq}\right) \rightleftharpoons {\mathrm{Cu}}^{+}\left(\mathrm{aq}\right) + \mathrm{Cu}\left(\mathrm{s}\right)$

choose correct E° for above reaction if

${\mathrm{E}}_{{\mathrm{Cu}}^{2+}/\mathrm{Cu}}^{°}= 0.34 \mathrm{V} \mathrm{and}\hspace{0.17em}{\mathrm{E}}_{{\mathrm{Cu}}^{2+}/{\mathrm{Cu}}^{+}}^{°} = 0.15 \mathrm{V}$

• -0.38 V

• + 0.49 V

• + 0.38 V

• -0.19 V

The number of electrons required to reduce 4.5 × 10^-5 of Al is

• 1.03 × 10¹⁸

• 3.01 × 10¹⁸

• 4.95 × 10²⁶

• 7.31 × 10²⁰