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How many electrons would be required to deposit $6.35 g$ of copper at the cathode during the electrolysis of an aqueous solution of copper sulphate?
(Atomic mass of copper $= 63.5 u {,N}_{A} =$ Avogadro’s constant):-

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Important Questions on Electrochemistry

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Alpha Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>Exercise-3>Q 44

298 K

, the standard reduction potentials are

1.51 V

for

{M n O}_{4}^{-} | M n^{2 +}

1.36 V

for

C l_{2} | C l^{-}

1.07 V

for

B r_{2} | B r^{-}

0.54 V

for

I_{2} | I^{-}

. At

pH = 3

, permanganate is expected to oxidize:

(\frac{R T}{F} = 0.059)

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Alpha Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>Exercise-3>Q 46

What is the standard reduction potential $(E °)$ for ${Fe}^{3 +} \to Fe$ ? Given that:
${Fe}^{2 +} + 2 e^{-} \to Fe; {E^{\circ}}_{{Fe}^{2 +} / Fe} = - 0.47 V$
${Fe}^{3 +} + e^{-} \to {Fe}^{2 +}; E °_{{Fe}^{3 +} / {Fe}^{2 +}} = + 0.77 V$

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Alpha Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>Exercise-3>Q 48

To find the standard potential of

M^{3 +} ∣ M

electrode, the following cell is constituted :

Pt | M | M^{3 +} (0.001 mol L^{- 1}) ||{Ag}^{+} (0.01 mol L^{- 1})| {Ag}^{+} (0.01 {molL}^{- 1})| Ag

The emf of the cell is found to be

0.421 volt

298 K

. The standard potential of half reaction

M^{3 +} + 3 e^{-} \to M

298 K

will be (Given

E_{{Ag}^{*} / Ag}^{O}

298 K = 0.80 volt

)

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Alpha Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>Exercise-3>Q 49

When an electric current is passed through acidified water, 112 mL of hydrogen gas at N.T.P was collected at the cathode in 965 seconds. The current passed, in ampere, is:

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Alpha Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>Exercise-3>Q 50

When 9.65 ampere current was passed for 1.0 hour into nitrobenzene in acidic medium, the amount of p-aminophenol produced is:

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Alpha Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>Exercise-3>Q 51

The anodic half-cell of lead-acid battery is recharged using electricity of

0 .05

Faraday. The amount of

{PbSO}_{4}

electrolyzed in

g

during the process is: (Molar mass of

{PbSO}_{4} = 303 g {mol}^{- 1}

)

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Alpha Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>Exercise-3>Q 52

If the standard electrode potential for a cell is

2 V

300 K,

the equilibrium constant

(K)

for the reaction.

Zn (s) + {Cu}^{2 +} (aq) ⇌ {Zn}^{2 +} (aq) + Cu (s)

300 K

is approximately:

(R = 8 {JK}^{- 1} {mol}^{- 1}, F = 96000 C {mol}^{- 1})

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Alpha Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>Exercise-3>Q 53

Consider the following reduction processes

{Zn}^{2 +} + 2 e^{-} \to Zn (s); E^{o} = - 0.76 V

{Ca}^{2 +} + 2 e^{-} \to Ca (s); E^{o} = - 2.87 V

{Mg}^{2 +} + 2 e^{-} \to Mg (s); E^{o} = - 2.36 V

{Ni}^{2 +} + 2 e^{-} \to Ni (s); E^{o} = - 0.25 V

The reducing power of the metals increases in the order

How many electrons would be required to deposit 6.35g of copper at the cathode during the electrolysis of an aqueous solution of copper sulphate? (Atomic mass of copper =63.5u,NA= Avogadro’s constant):-

Important Questions on Electrochemistry

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How many electrons would be required to deposit $6.35 g$ of copper at the cathode during the electrolysis of an aqueous solution of copper sulphate?
(Atomic mass of copper $= 63.5 u {,N}_{A} =$ Avogadro’s constant):-