The electrode potential of Cu electrode dipped in 0.025 M CuSO₄ solution at 298 K is:

(standard reduction potential of Cu = 0.34 V)

1. 0.047 V

2. 0.293 V

3. 0.35 V

4. 0.387 V

\(Cu(s)|Cu^{+2}(10^{-3} \ M) \ || \ Ag^{+}(10^{-5} \ M)|Ag(s)\)
if \(E_{Cu^{+2}/Cu}^{o} \ = \ +0.34 \ V\), and \(E_{Ag^{+}/Ag}^{o} \ = \ +0.80 \ V\)
E_cell will be: 

1. 0.46 V
2. \(0.46-\frac{RT}{2F}ln10^{7}\)
3. \(0.46+\frac{RT}{2F}ln10^{7}\)
4. \(0.46-\frac{RT}{2F}ln10^{2}\)

Consider the following cell reaction 

2Fe(s) + ${\mathrm{O}}_2$(g) + 4${\mathrm{H}}^{+}$(aq) $\to$ 2${\mathrm{Fe}}^{2+}$(aq) + 2${\mathrm{H}}_2\mathrm{O}$(l)

E° = 1.67 V, At [${\mathrm{Fe}}^{2+}$] = 10${}^{-3}$ M, ${\mathrm{P}}_{{\mathrm{O}}_2}$ = 0.1 atm and pH = 3, the cell potential at 25 °C is : 

1. 1.27 V

2. 1.77 V

3. 1.87 V

4. 1.57 V

The specific conductivity of a saturated solution of KI₃ is 4.59 × 10^-6 ohm^-1 cm^-1 and it's molar conductance is 1.53 ohm^-1 cm² mol^-1. The K_sp Of KI₃ will be : 

1. 4 x 10^-12

2. 27 x 27 x 10^-9

3. 9 x 10^-6

4. 4 x 10^-6

A 100.0 mL dilute solution of Ag⁺ is electrolyzed for 15.0 minutes with a current of 1.25 mA and the silver is removed completely. The initial [Ag⁺] is :-

1. 2.32 x 10${}^{-1}$ M

2. 2.32 x 10${}^{-4}$ M

3. 2.32 x 10${}^{-5}$ M

4. 1.17 x 10${}^{-4}$ M

Consider the change in the oxidation state of Bromine corresponding to different emf values as shown in the diagram below:

\(\small{BrO_4^-\ \overset{1.82V}{\longrightarrow}\ BrO_3^-\ \overset{1.5V}{\longrightarrow} HBrO\ \overset{1.595V}{\longrightarrow}\ Br_2 \overset{1.0652V}{\longrightarrow}\ Br^-}\) 
Then the species undergoing disproportionation is:-

On electrolysis of dilute sulphuric acid using Platinum (Pt) electrode, the product obtained at the anode will be:

1. Oxygen gas

2. ${\mathrm{H}}_2\mathrm{S}$ gas

3. ${\mathrm{SO}}_2$ gas

4. Hydrogen gas 

A fuel cell develops an electrical potential from the combustion of butane at 1 bar and 298 K 

C₄H₁₀(g) + 6.5O₂(g) → 4 CO₂(g) + 5H₂O(l); E^o  of a cell is: 

(Given \(\Delta G^{o}\) \(= - 2746  k J / m o l e\) )

1. 4.74 V

2. 0.547 V

3. 4.37 V

4. 1.09 V

Which of the following is most likely to occur when a gas X at 1 atm is bubbled through a solution containing 1 M Y⁻ and 1 M Z⁻ at 25 °C, if the standard reduction potentials follow the order Z > Y > X?

$∆\mathrm{G}°$ for the reaction given below is: 

$\frac{1}{2}\underset{}{\mathrm{A}\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>}+\frac{3}{2}\underset{}{\mathrm{B}\left(\mathrm{g}\right)<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>}\rightleftharpoons \underset{}{\mathrm{C}\left(\mathrm{g}\right)}$

(${\mathrm{K}}_{\mathrm{eq}}=826<mspace\; width="1em"></mspace>{\mathrm{atm}}^{-1}<mspace\; width="1em"></mspace>\mathrm{at}<mspace\; width="1em"></mspace>298<mspace\; width="1em"></mspace>\mathrm{K}$)

1. -8.32 kJ

2. 8.32 kJ

3. 16.64 kJ

4. -16.64 kJ