In a half-cell containing $\left[T{l}^{3+}\right] = 0.1 M and [T{l}^{+} ] = 0.01 M,$ the cell potential is – 1.2496 V for the reaction $T{l}^{+}\to T{l}^{3+} + 2e^{-}$  The standard reduction potential of the $T{l}^{+} /T{l}^{3+}$ couple at $25°C$ is

(1) 1.44 V                                          

(2) 0.61 V

(3) 2.44 V                                          

(4) 1.22 V

Given cell: 

Pt(s)|H₂(g)(P = 1 atm)| CH₃COOH(0.1 M), HCl(0.1 M) || KCl(aq)|Hg₂Cl₂(s)|Hg

EMF of the cell is found to be 0.045 V at 298 K and the temperature coefficient is 3.4×10^-4 V K^-1. The cell entropy change of the following cell is : 

[Given K_a CH₃COOH = 10^-5  M]

1. 70.8 J K⁻¹ mol⁻¹                      

2. 65.2 J K⁻¹ mol⁻¹

3. 79.2 J K⁻¹ mol⁻¹                  

4. 83.5 J K⁻¹ mol⁻¹

A dilute solution of $H_2 S{O}_4$ was electrolysed by passing a current of 2 amp. The time required for formation of 0.5 mole of oxygen is

(1) 26.8 hours                                    

(2) 13.4 hours

(3) 6.7 hours                                      

(4) 28.6 hours

The standard reduction potentials for $M{n}^{3+}/M{n}^{2+}$ and $Mn{O}_2 /M{n}^{3+}$ couples in acid medium at $25°C$ are 1.50 V and 1.00 V respectively. The following reaction:

$2M{n}^{3+} + 2H_{2}O \to M{n}^{2+} + Mn{O}_2 + 4H^{+} is$

(1) reversible                                             

(2) non-spontaneous

(3) spontaneous                                         

(4) irreversible

In the following electrochemical cell, $M|M^{+} || X^{-}|X,$ the standard reduction potentials are $E{°}_{M+/M}= 0.52 V$ and $E{°}_{X/X^{-}} = 0.42 V at 25°C.$ Which one of the following statements is correct ?

$\left(1\right) M + X \to M^{+} + X^{-} is spon\tan eous$              

$\left(2\right) M^{+} + X^{-} \to M + X is spon\tan eous$

$\left(3\right) E_{cell} = 0.77 V$                                              

$\left(4\right) E_{cell}= – 0.77 V$

1If a 100 mL solution of 0.1M HBr is titrated using a very concentrated solution of NaOH, when the conductivity (specific conductance) of the solution at the equivalence point will 3e (assume volume change is negligible due to addition of NaOH). Calculate your answer in terms of ${10}^{-1}S{m}^{-1},$

$\left[Given {{\wedge }^{°}}_{\left(N{a}^{+}\right)}=8\times {10}^{-3}S{m}^{2}mo{l}^{-1} {{\wedge }^{°}}_{\left(B{r}^{-}\right)}=4\times {10}^{-3}S m^2 mo{l}^{-1}\right]$

(1) 6                               

(2) 12

(3) 15                             

(4) 24

The volume of gases liberated at STP when a charge of 2F is passed through aqueous solution of sodium phosphate, is :

1. 11.2L                                           

2. 44.8L

3. 33.6L                                           

4. 22.4L

It is desired to convert the energy derived from the combustion of propane into electrical energy, via a fuel cell. Given that the standard free energies of formation of $C_3{H}_8 \left(g\right), H_{2}O\left(l\right) and C{O}_2 \left(g\right)$ are -23.5, -237.2 and -394.4 $kJ mo{l}^{-1}$ respectively, calculate the standard EMF of the propane fuel cell.

(1) 1.10 V                                           

(2) 2.10V

(3) 3.12 V                                           

(4) 4.12 V

The temperature coefficient of a standard Cd-cell is $–5.0 \times {10}^{-5} V{k}^{-1}$ whose emf at $25°C$ is 1.018 V. During the cell operation, the temperature will -

(1) increase                                      

(2) decreases

(3) either                                         

(4) remains constant

Na-amalgam is prepared by electrolysis of NaCl solution using liquid Hg as a cathode. How

long should the current of 10 amp. is passed to produce 10% Na – Hg on a cathode of 10

gm Hg. (atomic mass of Na = 23).

(A) 7.77 min.                                               

(B) 9.44 min.

(C) 5.24 min.                                               

(D) 11.39 min.