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An electrochemical cell is set up as: Pt; (1 atm)|HCl(0.1 M)|| (0.1 M)| (1 atm); Pt. The e.m.f. of this cell will not be zero, because
(a)acids used in two compartments are different
(b)e.m.f. depends on molarities of acids used
(c)the temperature is constant
(d)pH of 0.1 M HCl and 0.1 M is not same

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Important Questions on Redox Reactions and Electrochemistry
MEDIUM
For the following electrochemical cell at
when
Given:
The value of is -

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The pressure of required to make the potential of hydrogen electrode zero in pure water at 298 K is:

MEDIUM
The correct representation of Nernst’s equation for half- cell reaction is

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The electrode potential of a hydrogen electrode at is

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In the cell, the cell potential is when a molar solution is used. The standard electrode potential of electrode is:
(Given, at )

MEDIUM
For the given cell;
change in Gibbs energy is negative, it :

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For an electrochemical cell the ratio when this cell attains equilibrium is _______.
(Given: )

MEDIUM
Find the electrode potential for the given half-cell reaction given below at .
(Given, , temperature , oxygen is under standard atmospheric pressure of )

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In the electrochemical cell:
the emf of this Daniel cell is . When the concentration is changed to and that of changed to the emf changes to . From the following, which one is the relationship between and ? (Given, )

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The standard cell potential for is 1.10 V. When the cell is completely discharged, is closest to

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At , the standard reduction potentials are for , for , for , for . At , permanganate is expected to oxidize:

MEDIUM
The voltage of the cell consisting of and electrodes is at standard condition at . What is the voltage if the electrolyte consists of .
Given that,

MEDIUM
The electrode potentials for and are and respectively. The value of will be:

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The photoelectric current from Na (work function, ) is stopped by the output voltage of the cell
the of aq. required to stop the photoelectric current from , all other conditions remaining the same, is (to the nearest integer).
Given

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and are the emf of the following three galvanic cells respectively
(i)(ii)
(iii)
Which of the following is true?

MEDIUM
The of a galvanic cell consisting of two hydrogen electrodes is . If the solution of one of the electrodes has , the at the other electrode is:

MEDIUM
Given and .
The equilibrium constant for the reaction taking place in galvanic cell consisting of above two electrodes is

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What would be the electrode potential for the given half-cell reaction at

MEDIUM
To find the standard potential of electrode, the following cell is constituted:
The emf of the cell is found to be at . The standard potential of half-reaction at will be:
(Given: at )

HARD
For the electrochemical cell, the standard emf of the cell is at When the concentration of is changed to the cell potential changes to at The value of is ________.
(given, where is the Faraday constant and is the gas constants, )

