The number of electrons that have a total charge of 9650 coulombs is_______.

Faraday constant is defined as_______.

While charging lead storage battery _______.

Among the following cells
I) Leclanche cell
II) Nickel – Cadmium cell
III) Lead storage battery
IV) Mercury cell
Primary cells are ____.

The equivalent conductance of M/36 solution of a weak monobasic acid is 6 mho cm² equivalent^-1 and at infinite dilution is 400 mho cm² equivalent^-1. The dissociation constant of this acid is ______.

For the cell reaction
2Fe³⁺(aq) + 2l⁻(aq) \(\rightarrow\)2Fe²⁺ (aq) + 1₂ (aq)
E^o_cell = 0.24V  = at 298K. The standard Gibbs energy (Δ, G^o) of the cell reactions is:

Pick out the correct statement regarding resistance of an electrolytic solution ________.

Using the data given below find out the strongest reducing agent ______.
\({ E }_{ { Cr }_{ 2 }{ O }_{ 7 }^{ 2- } }^{ o }{ Cr }^{ 3+ }=1.33V{ ,E }_{ { Cl }_{ 2 }{ / }{ Cl }^{ - } }^{ o }=1.36V\)
\({ E }_{ { Mn }O_{ 4 }^{ - } }^{ 0 }/{ Mn }^{ 2+ }=1.51V,{ E }_{ { Cr }^{ 3+ }/Cr }^{ o }=-0.74V\)

Faraday's laws of electrolysis are related to ______.

According to Faraday's first law m = ZIt, where Z is ______.

If 0.2 ampere can deposit 0.1978 g of copper in 50 minutes, how much of copper will be deposited by 600 coulombs?

Calculate the standard emf of the cell, provided the standard reduction potentials of cathode and anode are -0.763 V and 0.80V.

The electrical energy produced by a cell equals _______.

The cell voltage depends on _______.

\({ \Lambda }_{ { NH }_{ 4 }OH }^{ o }\) is _______.

Why does conductivity of a solution decrease on dilution of the solution.

Describe the electrolysis of molten NaCl using inert electrodes

Why is anode in galvanic cell considered to be negative and cathode positive electrode?

The resistance of a conductivity cell is measured as 190 Ω using 0.1M KCl solution (specific conductance of 0.1M KCl is 1.3 Sm^-1). When the same cell is filled with 0.003 M sodium chloride solution, the measured resistance is 6.3KΩ. Both these measurements are made at a particular temperature. Calculate the specific and molar conductance of NaCl solution.

Derive the unit of specific conductance.

For a uni - univalent electrolyte write the Debye - Huckel Onsager equation

Molar conductivity increases with dilution. Is the above statement true? Justify your answer

Apply Kohlrausch's law and determine the limiting molar conductivity of
(i) BaCl₂
(ii) AI₂(SO₄)₃

What is the emf developed by a single lead storage battery?

The standard reduction potentials of Fe³⁺ / Fe and Fe²⁺ / Fe electrode system are -0.035 V and -0.44 V respectively. Predict which of the two oxidations is easy. Fe³⁺ / Fe and Fe²⁺ / Fe

The conductivity of a 0.01M solution of a 1 :1 weak electrolyte at 298K is 1.5\(\times\)10^-4 S cm⁻¹.
i) molar conductivity of the solution
ii) degree of dissociation and the dissociation constant of the weak electrolyte
Given that
\(\lambda^{0}_{cation}=248.2 \ S\) cm² mol^-1
\(\lambda^{0}_{anlon}=51.8 \ S\) cm² mol^-1

Why is AC current used instead of DC in measuring the electrolytic conductance?

Can Fe³⁺ oxidises Bromide to bromine under standard conditions?
Given: \({ E }_{ { Fe }^{ 3+ }|{ Fe }^{ 2+ } }^{ 0 }=0.771V\); \(\\ { E }^{0}_{ { Br }_{ 2 }|{ Br }^{ - } }=1.09V\).

Two metals M₁ and M₂ have reduction potential values of -xV and +yV respectively. Which will liberate H₂ and H₂SO₄.

Define molar conductance.

What is the oxidation and reduction half cell in a Daniel cell?

Give the oxidation and reduction half cell reaction taking place in the Daniel cell.

Explain the reactions taking place in the anode and cathode of a lead storage battery.

Define Faraday.

Draw a neat diagram of Leclanche cell and mark the parts.

Derive an expression for Nernst equation.

0.5 F of electric current was passed through 5 molar solution of AgNO₃, CuSO₄ and AICl₃ connected in series. Find out the concentration of each of the electrolyte after the electrolysis.

Write the Nernst equation for the half cell Zn²⁺_(aq)/ Zn_(s)

If E₁ = 0.5 V corresponds to Cr³⁺+ 3e^- ➝ Cr_(s) and E₂ = 0.41V corresponds to Cr³⁺+ e^- ➝ Cr²⁺ reactions, calculate the emf (E₃) of the reaction Cr²⁺+ 2 e^- ➝ Cr_(s)

Calculate the emf of the cell having the cell reaction 2Ag⁺ + Zn ⇌ 2Ag + Zn²⁺ and E^o_cell = 1.56 V at 25°C when concentration of Zn²⁺ = 0.1 M and Ag⁺ = 10 M in the solution.
\([{ E }_{ cell }={ E }_{ cell }^{ o }-\frac { RT }{ nF } In\frac { [{ Zn }^{ 2+ }] }{ [{ Ag] }^{ 2 } } ]\)

Derive a relationship between dissociation constant K_a and molar conductivity \({ \Lambda }_{ m }\)

Write an account on cell terminology.