A solution of Ni(NO₃)₂ is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of Ni is deposited at the cathode?

The resistance of a cell containing 0.001M KCl solution at 298 K is 1500 Ω. The conductivity is 0.146 × 10^–3 S cm^–1. The cell constant would be-

$1. 0.12 {\mathrm{cm}}^{-1}$

$2. 0.56 {\mathrm{cm}}^{-1}$

$3. 0.22 {\mathrm{cm}}^{-1}$

$4. 1.36 {\mathrm{cm}}^{-1}$

The number of Faradays required to produce 20.0 g of Ca from molten CaCl₂ is-

Three electrolytic cells A, B, C containing solutions of ZnSO₄, AgNO_3, and CuSO₄, respectively are connected in series. A steady current of 1.5 amperes was passed through them until 1.45 g of silver was deposited at the cathode of cell B. The current flow time is-

If a current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons would flow through the wire?

$$\begin{gathered} 1. 2.35 \times {10}^{-22} \\ 2. 2.25 \times {10}^{22} \\ 3. 1.34 \times {10}^{21} \\ 4. 3.16 \times {10}^{24} \end{gathered}$$

What is the quantity of electricity in coulombs needed to reduce 1 mol of ${\mathrm{Cr}}_2{\mathrm{O}}_7^{2-}$? Consider the reaction: ${\mathrm{Cr}}_2{\mathrm{O}}_7^{2-} + 14{\mathrm{H}}^{+} +\hspace{0.17em}6{\mathrm{e}}^{-} \to 2{\mathrm{Cr}}^{+3 }+ 7{\mathrm{H}}_2\mathrm{O}$

What is the potential of hydrogen electrode in contact with a solution whose pH is 10?

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

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

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 $E_{cell}^{⊝}$= 0.236 V at 298 K.

The equilibrium constant of the cell reaction is : 

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

The correct statement about the given galvanic cell equation is -

Zn_(s) + 2Ag⁺­­­_(aq) → Zn²⁺_(aq) + 2Ag_(s)

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

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

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

Electrode potential for Mg electrode varies according to the equation .${\mathrm{E}}_{{\mathrm{Mg}}^{2+}| \mathrm{Mg}}={\mathrm{E}}_{{\mathrm{Mg}}^{2+}|\mathrm{Mg}}^0-\frac{0.059}{2}\log \frac{1}{\left[{\mathrm{Mg}}^{2+}\right]}$ .

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

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 : 

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

An electrochemical cell can behave like an electrolytic cell when -

The incorrect statement about the solution of electrolytes is : 

$\begin{array}{l}{E}_{{\mathrm{Cr}}_2{\mathrm{O}}_7^{2-}/{\mathrm{Cr}}^{3+}}^{⊝}=1.33\mathrm{V} ; E_{{\mathrm{Cl}}_2/{\mathrm{Cl}}^{-}}^{\ominus }=1.36\mathrm{V}\\ E_{\mathrm{Mn}{O}_4^{-}/{\mathrm{Mn}}^{2+}}^{⊝}=1.51\mathrm{V} ; E_{{\mathrm{Cr}}^{3+}/\mathrm{Cr}}^{\ominus }=-0.74\mathrm{V}\end{array}$

Use the data give above, the most stable oxidized species is : 

The quantity of charge required to obtain one mole of aluminium from Al₂O₃ is :

The cell constant of a conductivity cell-

Correct statement about charging of the lead storage battery is -

${{\mathrm{\Lambda }}_{\mathrm{m}}^{°}}_{\left({\mathrm{NH}}_4\mathrm{OH}\right)}$ is equal to -

In the electrolysis of concentrated aqueous sodium chloride solution, the  half cell reaction will occur at the anode is : 

Match the terms given in Column I with the items given in Column II.

Codes

          A          B          C           D

Assertion: Current stops flowing when E_cell = 0.

Reason: Equilibrium of the cell reaction is attained.

Assertion: Copper sulphate can be stored in a zinc vessel.

Reason: Zinc is less reactive than copper.

In a typical fuel cell, the reactants (R) and product (P) are :-

The Gibb's energy for the decomposition of $A{l}_2{O}_3$ at $500°C$ is as follows: 

$\frac{2}{3}A{l}_2{O}_3\to \frac{4}{3}Al + O_2;∆rG = +960 kJ mo{l}^{-1}$

The potential difference needed for the electrolytic reduction of aluminium oxide
($A{l}_2{O}_3$) at $500°C$ is at least,

Molar conductivities $(\wedge {°}_m)$ at infinite dilution of NaCl, HCl and $C{H}_{3}COONa$ are 126.4, 425.9 and 91.0 S $c{m}^2 mo{l}^{-1}$ respectively. $(\wedge {°}_m)$  for $C{H}_{3}COOH$  will be: