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The reaction : \( \tfrac{1}{2}\mathrm{H_{2(g)}} + \mathrm{AgCl_{(s)}} \longrightarrow \mathrm{H^+_{(aq)}} + \mathrm{Cl^-_{(aq)}} + \mathrm{Ag_{(s)}} \)
Occurs in which of the following galvanic cell :

Fuel cell, using hydrogen and oxygen as fuels,
A. has been used in spaceship
B. has as an efficiency of \( 40\% \) to produce electricity
C. uses aluminum as catalysts
D. is eco-friendly
E. is actually a type of Galvanic cell only
Choose the correct answer from the options given below:

The standard reduction potentials at \( 298 \, \text{K} \) for the following half cells are given below:
\( \text{Cr}_2\text{O}_7^{2-} + 14\text{H}^{+} + 6e^{-} \rightarrow 2\text{Cr}^{3+} + 7\text{H}_2\text{O}, \, E^{\circ} = 1.33 \, \text{V} \)
\( \text{Fe}^{3+} (\text{aq}) + 3e^{-} \rightarrow \text{Fe}, \, E^{\circ} = -0.04 \, \text{V} \)
\( \text{Ni}^{2+} (\text{aq}) + 2e^{-} \rightarrow \text{Ni}, \, E^{\circ} = -0.25 \, \text{V} \)
\( \text{Ag}^{+} (\text{aq}) + e^{-} \rightarrow \text{Ag}, \, E^{\circ} = 0.80 \, \text{V} \)
\( \text{Au}^{3+} (\text{aq}) + 3e^{-} \rightarrow \text{Au}, \, E^{\circ} = 1.40 \, \text{V} \)
Consider the given electrochemical reactions,
The number of metal(s) which will be oxidized by \( \text{Cr}_2\text{O}_7^{2-} \), in aqueous solution is _______.

One of the commonly used electrode is calomel electrode. Under which of the following categories, calomel electrode comes?

The mass of silver (Molar mass of \( \mathrm{Ag} : 108 \, \text{g mol}^{-1} \)) displaced by a quantity of electricity which displaces \( 5600 \, \text{mL} \) of \( \mathrm{O_2} \) at S.T.P. will be ________ \( \text{g} \).

The amount of electricity in Coulomb required for the oxidation of \( 1 \, \text{mol} \) of \( \text{H}_2\text{O} \) to \( \text{O}_2 \) is ______ \( \times 10^{5} \, \text{C} \).

The hydrogen electrode is dipped in a solution of \( \mathrm{pH} = 3 \) at \( 25^\circ \mathrm{C} \). The potential of the electrode will be — __________ × \( 10^{-2} \) V.
\(\displaystyle
\left(\frac{2.303\,RT}{F} = 0.059\,\mathrm{V}\right) \)

Identify the factor from the following that does not affect electrolytic conductance of a solution.

The emf of cell is \( 0.83 \, \mathrm{V} \) at \( 298 \, \mathrm{K} \). It could be increased by:

The value of conductivity of some materials at \( 298.15 \, \text{K} \) in \( \text{S m}^{-1} \) are \( 2.1 \times 10^{3} \), \( 1.0 \times 10^{-16} \), \( 1.2 \times 10 \), \( 3.191 \), \( 1.5 \times 10^{-2} \), \( 1 \times 10^{-7} \), \( 1.0 \times 10^{3} \). The number of conductors among the materials is ________.

The metals that are employed in the battery industries are:
A. \( \mathrm{Fe} \)
B. \( \mathrm{Mn} \)
C. \( \mathrm{Ni} \)
D. \( \mathrm{Cr} \)
E. \( \mathrm{Cd} \)
Choose the correct answer from the options given below:

One Faraday of electricity liberates \( x \times 10^{-1} \) gram atom of copper from copper sulphate. \( x \) is ______.

The reaction at cathode in the cells commonly used in clocks involves.

For a strong electrolyte, a plot of molar conductivity against \( (\text{concentration})^{1/2} \) is a straight line, with a negative slope, the correct unit for the slope is:

For the electro chemical cell
\( \mathrm{M \;|\; M^{2+} \;||\; X \;|\; X^{2-}} \)
\( E^\circ_{(M^{2+}/M)} = 0.46 \, \text{V} \) and \( E^\circ_{(X/X^{2-})} = 0.34 \, \text{V} \)
Which of the following is correct?

A conductivity cell with two electrodes (dark side) are half filled with infinitely dilute aqueous solution of a weak electrolyte. If volume is doubled by adding more water at constant temperature, the molar conductivity of the cell will:

Molar ionic conductivities of divalent cation and anion are \( 57 \, \text{S cm}^2 \, \text{mol}^{-1} \) and \( 73 \, \text{S cm}^2 \, \text{mol}^{-1} \) respectively. The molar conductivity of solution of an electrolyte with the above cation and anion will be:

The molar conductivity for electrolytes A and B are plotted against \( c^{1/2} \) as shown below. Electrolytes A and B respectively are:

How can an electrochemical cell be converted into an electrolytic cell?

Consider the following redox reaction: \( \mathrm{MnO_4^-} + \mathrm{H^+} + \mathrm{H_2C_2O_4} \rightleftharpoons \mathrm{Mn^{2+}} + \mathrm{H_2O} + \mathrm{CO_2} \)
The standard reduction potentials are given as below \( (E^\circ_{\text{red}}) \):
\( E^\circ_{\mathrm{MnO_4^-/Mn^{2+}}} = +1.51 \, \text{V} \)
\( E^\circ_{\mathrm{CO_2/H_2C_2O_4}} = -0.49 \, \text{V} \)
In the equilibrium constant of the above reaction is given as \( K_{\mathrm{eq}} = 10^{x} \) , then the value of \( x = \) __________. (nearest Integer)

The potential for the given half cell at \( 298 \, \text{K} \) is (−) _______ \( \times 10^{-2} \, \text{V} \).
\( 2\mathrm{H}^+(\mathrm{aq}) + 2e^- \rightarrow \mathrm{H}_2(\mathrm{g}) \)
\( [\mathrm{H}^+] = 1 \, \text{M}, \; P_{\mathrm{H}_2} = 2 \, \text{atm} \)
[Given : \( 2.303 \, \frac{RT}{F} = 0.06 \, \text{V}, \; \log 2 = 0.3 \)]

The mass of zinc produced by the electrolysis of zinc sulphate solution with a steady current of \( 0.015 \, \mathrm{A} \) for \( 15 \) minutes is __________ \( \times 10^{-4} \, \mathrm{g} \). (Atomic mass of zinc \( = 65.4 \, \mathrm{amu} \))

The quantity of silver deposited when one coulomb charge is passed through \( \mathrm{AgNO_3} \) solution:

Which out of the following is a correct equation to show change in molar conductivity with respect to concentration for a weak electrolyte, if the symbols carry their usual meaning:

A constant current was passed through a solution of \( \mathrm{AuCl}_4^- \) ion between gold electrodes. After a period of \( 10.0 \) minutes, the increase in mass of cathode was \( 1.314 \, \text{g} \). The total charge passed through the solution is _______ \( \times 10^{-2} \, \text{F} \). (Given atomic mass of Au = \( 197 \))

What pressure \( \text{(bar)} \) of \( \mathrm{H_2} \) would be required to make emf of hydrogen electrode zero in pure water at \( 25^\circ \mathrm{C} \)?

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JEE Main 2024 5th April Evening Shift

The quantity of silver deposited when one coulomb charge is passed through \( \mathrm{AgNO_3} \) solution: