What will be the emf of the cell in which the following reaction takes place? Given ${\mathrm{E}}_{\mathrm{cell}}^{°} = 1.05 \mathrm{V}$

${\mathrm{Ni}}_{\left(\mathrm{s}\right)}+2{\mathrm{Ag}}^{+}(0.002 \mathrm{M}) \to {\mathrm{Ni}}^{2+}(0.160 \mathrm{M}) + 2{\mathrm{Ag}}_{\left(\mathrm{s}\right)}$

1. 0.80 V

2. 0.91 V

3. 0.45 V

4. 0.36 V

The cell in which the following reactions occurs:

$2{{\mathrm{Fe}}^{3+}}_{\left(\mathrm{aq}\right)}+2{{\mathrm{I}}^{-}}_{\left(\mathrm{aq}\right)}\to 2{{\mathrm{Fe}}^{2+}}_{\left(\mathrm{aq}\right)}+{\mathrm{I}}_{2\left(\mathrm{s}\right)}$ has  \(E_{cell}^{o}\) = 0.236 V at 298 K.

The equilibrium constant of the cell reaction is : 

$1.$ $9.57$ $\times$ ${10}^7$
$2.$ $8.43$ $\times$ ${10}^6$
$3.$ $3.68$ $\times$ ${10}^{-7}$
$4.$ $1.74$ $\times$ ${10}^5$

The molar conductivity of 0.025 mol L⁻¹ methanoic acid is 46.1 S cm² mol⁻¹.

What is the dissociation constant of methanoic acid? Given λ°(H⁺)= 349.6 S cm² mol⁻¹ and λ°(HCOO⁻) = 54.6 S cm² mol^-1

^{$1. 2.43 \times {10}^4 \mathrm{mol} {\mathrm{L}}^{-1}$
$2. 1.15 \times {10}^{-5} \mathrm{mol} {\mathrm{L}}^{-1}$
$3. 3.67 \times {10}^{-4} \mathrm{mol} {\mathrm{L}}^{-1}$
$4. 2.44 \times {10}^{-6 }\mathrm{mol} {\mathrm{L}}^{-1}$}

Mg_(s) | Mg²⁺_(0.001M) || Cu²⁺_{(0.0001 M)} | Cu_(s)

${\mathrm{E}}_{{\mathrm{Mg}}^{2+}/\mathrm{Mg}}^{\mathrm{o}}=-2.36 \mathrm{V}; {\mathrm{E}}_{{\mathrm{Cu}}^{2+}/\mathrm{Cu}}^{\mathrm{o}}=0.34\mathrm{V}$

The value of ${\mathrm{E}}_{\mathrm{cell} }$ for the above reaction is -

The cell that will measure the standard electrode potential of a copper electrode is:

The electrode potential for Mg electrode varies according to the equation

\(E_{Mg^{2+}/Mg}\ = \ E_{Mg^{2+}/Mg}^{o} \ - \ \frac{0.059}{2}log\frac{1}{[Mg^{2+}]}\) 

The graph of E_{Mg²⁺ / Mg} vs log [Mg²⁺] among the following is:

1.		2.
3.		4.

The correct statement among the following options is: 

The difference between the electrode potentials of two electrodes when no current is drawn through the cell is called:
1. Cell potential.
2. Cell emf.
3. Potential difference.
4. Cell voltage.

The incorrect statement about an inert electrode in a cell is:

An electrochemical cell can behave like an electrolytic cell when -

1. E_cell = 0

2. E_cell > E_ext

3. E_ext > E_cell

4. E_cell = E_ext