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TEST - 1 Electrochemistry

This document contains a test with multiple choice and numerical questions regarding concepts in electrochemistry. It includes 5 questions worth 2 marks each about electrode potentials, molar conductivity graphs, types of cells, and calculating potentials. It also includes 5 questions worth 3 marks each involving depicting galvanic cells, calculating molar conductivity, and cell potentials. Finally, it contains 5 questions worth 5 marks each involving calculating dissociation constants from conductivity, determining mass deposited in electrolytic cells, defining electrochemical terms, and calculating cell emfs.

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431 views2 pages

TEST - 1 Electrochemistry

This document contains a test with multiple choice and numerical questions regarding concepts in electrochemistry. It includes 5 questions worth 2 marks each about electrode potentials, molar conductivity graphs, types of cells, and calculating potentials. It also includes 5 questions worth 3 marks each involving depicting galvanic cells, calculating molar conductivity, and cell potentials. Finally, it contains 5 questions worth 5 marks each involving calculating dissociation constants from conductivity, determining mass deposited in electrolytic cells, defining electrochemical terms, and calculating cell emfs.

Uploaded by

carsk403
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
Available Formats
Download as PDF, TXT or read online on Scribd
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TEST- 1

Chapter -3
Electrochemistry
M.M:- 50

➢ Answer the following questions ( 2 marks each)

Q-1 A zinc rod is dipped in 0.1 M solution of ZnSO4. The salt is 95%
Dissociated at this dilution at 298 K.Calculate the electrode potential.
[ EOZn2+/ Zn = - 0.76V ]
Q-2 Explain with a graph the variation of molar conductivity of a strong
Electrolyte with dilution.
Q-3 Write the name of the cell which is generally used in hearing aids
Write the reactions taking place at the anode and cathode of this
Cell.
Q-4 Calculate the potential of hydrogen electrode in contact with a solution
Whose pH is 10.
Q-5 If a current of 0.5 ampere flows through a metallic wire for 2 hours,
Then how many electrons would flow through the wire?

➢ Answer the following questions ( 3 marks each)

Q-1 Consider the following reaction:


Cu + 2 Ag+ (aq) 2 Ag (s) + Cu2+ ( aq)
1. Depict the galvanic cell in which the reaction taking place.
2. Give the direction of flow of current.
3. Write the half cell reactions taking place at cathode and anode.

Q-2 The conductivity of 0.20 M solution of KCl at 298 K is 0.0248 S cm-1.


Calculate its molar conductivity.

Q-3 The electrical resistance of a column of 0.05 M of NaOH solution of


Diameter 1 cm and length 50 cm is 5.55 x 103Ω. Calculate its
Resistivity, conductivity and molar conductivity.

Q-4 Calculate the emf of the following cell at 250C.


Zn Zn2+ (0.001M) H+ (0.01) H2 (g)(1 bar) Pt(s)
EO(Zn2+ / Zn) = -0.76 V, EO(H+/H2 = 0.00V

Q-5 How much electricity in terms of faraday is required to produce :

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a. 20.0g of Ca from molten CaCl2
b. 40.0g of Al from molten Al2O3

➢ Answer the following questions ( 5 marks each)

Q-1 Conductivity of 0.00241 M acetic acid is 7.896 x 10-5 S cm-1. Calculate


its molar conductivity. If ΛOm, for acetic acid is 390.5 S cm2 mol-1, what
is its dissociation constant?

Q-2 Three electrolytic cells A, B, C containing solutions of ZnS04, AgNO3 and


CuS04, respectively are connected in series. A steady current of 1.5
amperes was passed through them until 45 g of silver deposited at the
cathode of call B. How long did the current flow? What mass of copper
and zinc were deposited?

Q-3 i. The conductivity of 0.001 mol L-1 Solution of CH3COOH is 3.905 x 10-5
S cm-1. Calculate its molar conductivity and degree of dissociation (α)
Given , λo (H+) = 349.6 Scm2mol-1 and λo (CH3COO-) = 40.9 Scm2mol-1

ii. Define electrochemical cell. What happens if external potential


applied becomes greater than EOcell of electrochemical cell?

Q-4 i. Define the following terms:


a. Limiting molar conductivity
b. Fuel cell
ii. Resistance of a conductivity cell filled with 0.1 mol L-1 KCl solution is
100 Ω. If the resistance of the same cell filled with 0.02 mol L-1 KCl
solution is 520 Ω, calculate the conductivity and molar conductivity
of 0.02 mol L-1 KCl solution. The conductivity of 0.1 mol L-1 KCl
solution is 1.29 x 10-2 Ω-1 cm-1.

Q-5 i. State faraday’s first law of electrolysis. How much charge in terms
Of faraday’s is required for the reduction of 1 mole of Cu2+ to Cu.
ii. Calculate emf of the following cell at 298 K.
Mg (s) Mg2+ (0.1M) Cu2+(0.01) Cu(s)
Given, EOcell = +2.71 V,
1F = 96500 C mol-1

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