Which of the following electrolytic solution has the least specific conductance?

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

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 ______.

A conductivity cell has been calibrated with a 0.01M, 1:1 electrolytic solution (specific conductance (k = 1.25 x 10^-3cm^-1) in the cell and the measured resistance was 800 Ω at 25^oC. The cell constant is ______.

Kohlraush's law is applied to calculate ________.

The specific conductance of a 0.01 M solution of KCI is 0.0014 ohm^-1 em^-1 at 25°C. Its equivalent conductance is ______.

The equivalent conductivity of CH₃COOH at 25°C is 80 ohm^-1 cm² eq^-1 and at infinite dilution 400 ohm^-1 cm^-1 eq^-1. The degree of dissociation of CH₃COOH is ______.

The important use of Kohlrausch's law is deducing the ______.

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

Which among the following has same equivalent and molar conductance?

Ionic conductance at infinite dilution of Al³⁺ and SO^2-₄ are 1890 ohm^-1 cm² gm equiv^-1 and 1600 ohm^-1 cm^-2 gm equiv^-1 respectively. The equivalent conductance is ______.

Which of the following statement is wrong with regard to galvanic cell?

Standard electrode potential of Sn⁴⁺ / Sn²⁺  couple is +0.15 V and that of Cr³⁺ / Cr is 0.85 V. When connected, the cell potential will be ______.

The cell in which electrical energy is used to bring about chemical change is known as _______.

The feasibility of a redox reaction can be predicted with the help of ________.

State Kohlrausch Law. How is it useful to determine the molar conductivity of weak electrolyte at infinite dilution.

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

A conductivity cell has two platinum electrodes separated by a distance 1.5 cm and the cross sectional area of each electrode is 4.5 sq cm. Using this cell, the resistance of 0.5 N electrolytic solution was measured as 15 Ω. Find the specific conductance of the solution.

On dilution of 0.1 M of Na₂SO₄, what will happen to its
(a) Conductance (C)
(b) Conductivity K
(c) Molar conductance \({ \Lambda }_{ m }\)
(d) Equivalent conductance \({ \Lambda }\)

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

What are the factors on which cell potential depends?

Higher the standard reduction potential lesser is corrosion. Give reason.

Define electrochemical equivalent.

What is single electrode potential?

Write the Nernst equation.

0.1M NaCl solution is placed in two different cells having cell constant 0.5 and 0.25 cm^-1 respectively. Which of the two will have greater value of specific conductance.

Reduction potential of two metals M₁ and M₂ are \(E^{0}_{M^{2+}_{1}|M_{1}} = -2.3V\) and \(E^{0}_{M^{2+}_{1}|M_{1}} = 0.2V\) Predict which one is better for coating the surface of iron. Given : \(\mathrm{E}_{\mathrm{Fe}^{2+} \mid \mathrm{Fe}}^{\circ}=-0.44 \mathrm{~V}\)

Answer the following question with regard to specific resistance.
(i) How is specific resistance represented?
(ii) What does specific resistance depend on?
(iii) What is the reciprocal of specific resistance? How is it denoted.
(iv) What is the unit of resitivity?

Define equivalent conductance.

How are electro chemical cells classified? Explain.

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

Write the cell representation of the galvanic cell in which the following reaction take place
\({ Zn }_{ (s) }+Cu{ SO }_{ 4 }\rightarrow { ZnSO }_{ 4 }+{ Cu }_{ (s) }\)
For the above cell. Identify the anode and cathode half cell.

Explain the IUPAC convention of representing a Galvanic cell.

Leclanche cell is a non-rechargeable cell. Answer the questions below with respect to Leclanche cell.
(i) Anode
(ii) Cathode
(iii) Electrolyte
(iv) Oxidation half cell reaction
(v) Reduction half cell reaction.

Define Faraday.

Calculate the standard emf of the cell: Cd|Cd²⁺||Cu²⁺|Cu and determine the cell reaction. The standard reduction potentials of Cu²⁺|Cu and Cd²⁺|Cd are 0.34V and -0.40 volts respectively. Predict the feasibility of the cell reaction.

Derive an expression for Nernst equation.

The electrochemical equivalent of an electrolyte is 2.35 gm amp^-1 sec^-1. Calculate I the amount of the substance deposited when 5 ampere is passed for 10 sec.

Specific conductance of 1M KNO₃ solution is oberved to be 5.55 x 10^-3 mho cm². What is the equivalent conductance of KNO₃ when one litre of the solution is used?

The standard reduction potential for the reaction Sn⁴⁺ + 2e^- ⟶ Sn²⁺ is + 0.15v. Calcuate the free energy change of the reaction.

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

How will you determine the conductivity of an electrolytic solution using a wheatstone, bridge?