At 25$°$C, the molar conductances at infinite dilution for the strong electrolytes NaOH, NaCl and BaCl₂ are 248 $\times$10^-4, 126 x 10^-4 and 280 x 10^-4 Sm² mol^-1 respectively, ${\mathrm{\lambda }}_{\mathrm{m}}^{\infty }$  Ba(OH)₂ in Sm² mol^-1 is

• 52.4 $\times$ 10^-4

• 524 $\times {10}^{-4}$

• 402 $\times {10}^{-4}$

• 262 $\times {10}^{-4}$

62.

The molar conductivities of KCl, NaCl and KNO₃ are 152, 128 and 111 S cm²mol^-1 respectively. What is the molar conductivity of NaNO₃?

• 101 S cm²mol^-1 

• 87 S cm²mol^-1 

• -101 S cm²mol^-1 

• -39 S cm²mol^-1 

The electrochemical cell stops working after sometime because

• electrode potential of both the electrodes becomes zero

• electrode potential of both the electrodes becomes equal

• one of the electrodes is eaten away

• the cell reaction gets reversed

The amount of electricity required to produce one mole of copper from copper sulphate solution will be

• 1 F

• 2.33 F

• 2 F

• 1.33 F

How long (in hours) must a current of 5.0 A be maintained to electroplate 60 g of calcium from molten CaCl₂ ?

• 27 h

• 8.3 h

• 11 h

• 16 h

For strong electrolytes the plot of molar conductance vs $\sqrt{\mathrm{C}}$ is

• parabolic

• linear

• sinusoidal

• circular

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

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