Beta Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>EXERCISE-1>Q 26

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Earn 100

Consider the reaction: $(T = 298 K)$

${Cl}_{2} (g) + 2 {Br}^{-} (aq) ⟶ 2 {Cl}^{-} (aq) + {Br}_{2} (aq)$

Determine the emf (in volts) of the cell, when $[{Cl}^{-}] = [{Br}_{2}] = [{Br}^{-}] = 0.01 M$ and ${Cl}_{2}$ gas is at $1 atm$ pressure.

( $E °$ for the above reaction is $= 0.29$ volt)

Enter only the numerical value in the box and exclude the units.

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Important Questions on Electrochemistry

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Beta Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>EXERCISE-1>Q 27

Three faradays of electricity was passed through an aqueous solution of iron

(II)

bromide. The mass of iron metal (at. mass

56

) deposited at the cathode is -

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Beta Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>EXERCISE-1>Q 29

Three moles of electrons are passed through three solutions in succession containing

{AgNO}_{3}, {CuSO}_{4}

and

{AuCl}_{3}

, respectively. The molar ratio of amounts of cations reduced at cathode will be:

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Beta Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>EXERCISE-1>Q 30

For the electrochemical cell,

$M | M^{+} | | X^{-} ∣ X, E_{M^{+} | M} ° = 0.44 V & E_{X | X^{-}} ° = 0.33 V$

From this data, one can deduce that :

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Beta Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>EXERCISE-1>Q 31

How many faradays are required to reduce one

mol

of

{MnO}_{4}^{-}

to

{Mn}^{2 +}

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Beta Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>EXERCISE-1>Q 32

${Cu}^{+} + e^{-} ⟶ Cu, E ° = x_{1} volt$

${Cu}^{2 +} + 2 e^{-} ⟶ Cu, E ° = x_{2} volt$

Then for ${Cu}^{2 +} + e^{-} ⟶ {Cu}^{+}$ , $E ° (volt)$ will be:

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Beta Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>EXERCISE-1>Q 33

Zn |{Zn}^{2 +} (C_{1}) ‖ {Zn}^{2 +} (C_{2})| Zn

for this cell

ΔG

is negative if

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Beta Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>EXERCISE-1>Q 34

Pt |\begin{array}{l} H_{2} & H^{+} \\ (p_{1}) & (1 M) \end{array} ‖ \begin{array}{l} H^{+} \\ (1 M) \end{array}| \begin{array}{l} H_{2} \\ (p_{2}) \end{array} Pt

, (where

p_{1}

and

p_{2}

are pressures) cell reaction will be spontaneous if:

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Beta Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>EXERCISE-1>Q 35

In an electrochemical cell that function as a voltaic cell :-