During the electrolysis of molten sodium chloride, the time required to produce 0.10 mol of chlorine gas using a current of 3 amperes is

If the E°_cell for a given reaction has a negative value, which of the following gives correct relationships for the values of $∆$G° and K_eq ?

The number of electrons delivered at the cathode during electrolysis by a current of 1 ampere in 60 seconds is (charge on electron = 1.60 x 10^-19 C)

Zinc can be coated on iron to produce galvanised iron but the reverse is not possible. It is because

The pressure of H₂ required to make the potential of H₂-electrode zero in pure water at

298 K is

A device that converts energy of combustion of fuels like hydrogen and methane, directly

into electrical energy is known as

The weight of silver (at. wt.= 108) displaced by a quantity of electricity which displaces 5600 mL of O₂ at STP will be : 

At 25° C molar conductance of 0.1 molar aqueous solution of ammonium hydroxide is

9.54 ohm¹cm²mol^-1 and at infinite dilution its molar conductance is 238 ohm¹cm²mol^-1.

The degree of ionisation of ammonium hydroxide at the same concentration and

temperature is

A button cell used in watches functions as following

Zn(s) + Ag₂O(s) + H₂O (l) $\rightleftharpoons$2Ag(s) + Zn²⁺(aq) + 2OH^-(aq)

If half cell potentials are

$$\begin{gathered} {{\mathrm{Zn}}^{2+}}_{\left(\mathrm{aq}\right)} +\hspace{0.17em}2{\mathrm{e}}^{-} \to {\mathrm{Zn}}_{\left(\mathrm{x}\right)}; {\mathrm{E}}^{\mathrm{o}} = -0.76\mathrm{V} \\ {\mathrm{Ag}}_2{\mathrm{O}}_{\left(\mathrm{s}\right)} + {\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{l}\right)} + 2{\mathrm{e}}^{-} \to 2{\mathrm{Ag}}_{\left(\mathrm{s}\right)} + 2{{\mathrm{OH}}^{-}}_{\left(\mathrm{aq}\right)}; \\ {\mathrm{E}}^{\mathrm{o}} = 0.34\mathrm{V} \end{gathered}$$

The cell potential will be

Limiting molar conductivity of NH₄OH (i.e Åm(NH₄OH)) is equal to:-

Kohlrausch's law states that at

The efficiency of a fuel cell is given by:

$$\begin{gathered} \left(\mathrm{a}\right) ∆\mathrm{H}/∆\mathrm{G} \left(\mathrm{b}\right) ∆\mathrm{G}/∆\mathrm{S} \\ \left(\mathrm{c}\right) ∆\mathrm{G}/∆\mathrm{H} \left(\mathrm{d}\right) ∆\mathrm{S}/∆\mathrm{G} \end{gathered}$$

A hypothetical electrochemical cell is shown below A l A⁺ (xM)l l B⁺ (yM) l B
The Emf measured is +0.20 V.The cell reaction is:-

The E° in the given diagram is,

At 298K the standard free energy of formation of H₂O(l) is –237.20kJ/mole while that of its ionisation into H+ iion and hydroxyl ions is 80 kJ/mole, then the emf of the following cell at 298 K will be

H₂(g,1 bar) | H⁺ (1M) || OH^–(1M) | O₂ (g, 1bar)

Which of the following cell can produce more electric work.

At what $\frac{\left[{\mathrm{Br}}^{\mathrm{-}}\right]}{\sqrt{\left[{\mathrm{CO}}_3^{2-}\right]}}$ does the following cell have its reaction at equilibrium?

Ag(s) | Ag₂CO₃(s) | Na₂CO₃ (aq) || KBr(aq) | AgBr(s) | Ag(s)

K_SP = 8 × 10^–12 for Ag₂CO₃ and K_SP = 4 × 10^–13 for AgBr

It is observed that the voltage of a galvanic cell using the reaction M(s) + xH⁺ $\underset{}{\overset{}{\to }}$ M^x+ + $\frac{x}{2}$ H₂ varies linearly with the log of the square root of the hydrogen pressure and the cube root of the M^x+ concentration. The value of x is

Acetic acid has K_a = 1.8 × 10^–5 while formic acid had K_a = 2.1 × 10^–4. What would be the magnitude of the emf of the cell

Pt(H₂) $\left|\begin{array}{l}0.1\mathrm{M} \mathrm{acetic} \mathrm{acid}+\\ 0.1\mathrm{M} \mathrm{sodium} \mathrm{acetate}\end{array}\right|\left|\begin{array}{l}0.1\mathrm{M} \mathrm{formic} \mathrm{acid}+\\ 0.1\mathrm{M} \mathrm{sodium} \mathrm{formate}\end{array}\right|$ Pt(H₂) at 25°C

Consider the cell Ag(s)|AgBr(s)|Br–(aq)||AgCl(s)|Cl–(aq)|Ag(s) at 25°C. The solubility product constants of AgBr & AgCl are respectively 5 × 10^–13 & 1 × 10^–10. For what ratio of the concentrations of Br^– & Cl^–ions would the emf of the cell be zero ?

Calculate the useful work of the reaction Ag(s) + 1/2Cl₂(g) $\underset{}{\overset{}{\to }}$ AgCl(s)

Given $\mathrm{E}{°}_{\mathrm{Cl}2/{\mathrm{Cl}}^{–}} = + 1.36 \mathrm{V}, \mathrm{E}{°}_{\mathrm{AgCl}/\mathrm{Ag},{\mathrm{Cl}}^{–}} = 0.22 \mathrm{V}$

If ${\mathrm{P}}_{{\mathrm{Cl}}_2}$ = 1 atmand T = 298 K

Which of these ions Cu⁺, Co³⁺, Fe²⁺ is stable in aqueous medium.

Given :E°_Cu2+/Cu+ = 0.15 volt ; E°_Cu+/Cu = 0.53 V ;E°_Co3+/Co2+ = 1.82 V ;

E°_Fe3+/Fe2+ = 0.77 V ;E°_Fe2+Fe = –0.44 V ;E°_O2,H+/H2O = 1.23 V

Select the correct statement if –

E°_Mg2+/Mg = –2.4V, E°_Sn4+/Sn2+ = 0.1 V, E°_{MnO4–,H+/Mn2+} = 1.5 V, E° _I2/I–= 0.5 V

Here,

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

A cell Ag | Ag⁺ || Cu⁺⁺ | Cu initially contains 2M Ag⁺ and 2M Cu⁺⁺ ions. The charger in cell potential after the passage of 10 amp current for 4825 sec is:

For the cell (at 298 K)

Ag(s) | AgCl(s) | Cl^–(aq) || AgNO₃(aq) | Ag(s)

Which of the following is correct –

Equivalent conductivity of ${\mathrm{Fe}}_2{\left({\mathrm{SO}}_4\right)}_3$is related to molar conductivity by the expression:

Assertion : In electrochemical cell, we cannot use $\mathrm{KCI}$ in the salt bridge if anodic or cathodic

                  compartment consists of ${\mathrm{Ag}}^{+}$ of ${\mathrm{Pb}}^{2+}$ ion.

Reason : Salt bridge is employed to maintain the electrical neutrality and to minimize the liquid-liquid

               junction potential.

What will be the quantity of iron deposited by ferrous and ferric ion by 1F (Fe = 56)

(D)The reaction for the cell,

$Zn | Z{n}^{2+} (1.0 M) || C{d}^{2+} (1.0 M) | Cd is-$

$\left(A\right) Cd \to C{d}^{2+}+ 2e^{-}$

$\left(B\right) Z{n}^{2+}\to Zn – 2e^{-}$

$\left(C\right) Cd + Z{n}^{2+}\to C{d}^{2+}+ Zn$

$\left(D\right) Zn + C{d}^{2+} \to Cd + Z{n}^{2+}$