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Electro Chemistry Chemistry - Electro Chemistry

Bihar Board (BSEB) - STD 12 Science - Chemistry (BSEB - English Medium). 57 questions in this chapter.

Question types

Electro Chemistry question types

57 questions across 6 question groups — pick any mix to generate a Chemistry paper with step-by-step answer keys.

57
Questions
6
Question groups
5
Question types
Sample Questions

Electro Chemistry questions

One sample from each question group in this chapter. Select any group above to see the full set with answer keys.

Q 1M.C.Q [1M]1 Mark
The electromotive force of the cell Zn | $ZnSO_{4}$ || $CuSO_{4}$ | Cu is 1.1 volt. Its cathode is:
  • A
    Zn
  • ✓
    Cu
  • C
    $ZnSO_{4}$
  • D
    $CuSO_{4}$

Answer: B.

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Q 3M.C.Q [1M]1 Mark
The best way to protect iron from rusting is:
  • ✓
    Making iron cathode
  • B
    Putting it in saline water
  • C
    (a) and (b) both
  • D
    None of these

Answer: A.

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Q 4M.C.Q [1M]1 Mark
Faraday's second law of electrolysis are related to:
  • A
    Atomic number of cation
  • B
    Atomic number of anion
  • ✓
    Equivalent weight of electrolyte
  • D
    Speed of Cation

Answer: C.

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Q 5M.C.Q [1M]1 Mark
How much charge is required for reduction of 1 mole of $Al^{3+}$ to Al?
  • ✓
    $3.0 \times 10^{5} C$
  • B
    $28.95 \times 10^{5} C$
  • C
    $289.5 \times 10^{5} C$
  • D
    $2895 \times 10^{5} C$

Answer: A.

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Q 61 Marks Question1 Mark
The cell in which the following reaction occurs: $Fe_{(aq)}^{3+} + 2I_{(aq)}^{-} \longrightarrow 2Fe_{(aq)}^{2+} + I_{2(s)}$ has $E_{cell}^{0} = 0.236 V$ at 298 K. Calculate the standard Gibbs energy of the cell reaction. (Given: $1 F = 96500 C mol^{-1}$)
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Q 11Short Answer Type Questions [2M]2 Marks
(a) Calculate $\Delta G^{0}$ for the reaction
$Zn(s) + Cu^{2+}(aq) \longrightarrow Zn^{2+}(aq) + Cu(s)$.
Given: $E^{0}$ for $Zn^{2+}/Zn = -0.76 V$ and
$E^{0}$ for $Cu^{2+}/Cu = +0.34 V$,
$R = 8.314 J K^{-1} mol^{-1}$,
$F = 96500 C mol^{-1}$.
(b) Give two advantages of fuel cells.
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Q 163 Marks Question3 Marks
$E_{\text {cell }}^0$ for the given redox reaction is 2.71 V
$Mg _{( s )}+ Cu _{(0.01 M )}^{2+} \longrightarrow \stackrel{2++ Cu _{( s )}}{ Mg _{(0.001 M )}^{2+}}$
Calculate $E_{\text {cell }}$ for the reaction. Write the direction of flow of current when an external opposite potential applied is
(i) less than 2.71 V and (ii) greater than 2.71 V .
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Q 173 Marks Question3 Marks
For the reaction $2AgCl_{(s)} + H_{2(g)}$ (1 atm) $\rightarrow$ $2Ag_{(s)} + 2H^{+} (0.1 M) + 2Cl^{-} (0.1M)$
$\Delta G^{0} = -43600 J$ at $25^{\circ}C$.
Calculate the emf of the cell. [$log 10^{-n} = -n$]
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Q 193 Marks Question3 Marks
Calculate $E _{ cell }^0$ for the following reaction at 298 K.
$2 Cr _{(s)}+3 Fe ^{2+}\left(0.1 M \rightarrow 2 Cr ^{3+}(0.01 M )+3 Fe _{(s)}\right.$
Given : $E _{\left( Cr ^{3+} / Cr \right)}^{\circ}=-0.74 V, E _{\left( Fe ^{2+} / Fe \right)}^{\circ}=-0.44 V$
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Q 20Long Answer Type Questions [5M]5 Marks
A steady current of 2 amperes was passed through two electrolytic cells X and Y connected in series containing electrolytes $FeSO_{4}$ and $ZnSO_{4}$ until 2.8 g of Fe deposited at the cathode of cell X. How long did the current flow? Calculate the mass of Zn deposited at the cathode of cell Y. (Molar mass: $Fe = 56 g mol^{-1}, Zn = 65.3 g mol^{-1}, 1 F = 96500 C mol^{-1}$)
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Q 254 Marks Questions4 Marks
(a) Out of the following pairs, predict with reason which pair will allow greater conduction electricity:
(i) Silver wire at $30^{\circ}C$ or silver wire at $60^{\circ}C.$
(ii) 0.1 M $CH_{3}COOH$ solution or 1 M $CH_{3}COOH$ solution.
(iii) KCl solution at $20^{\circ}C$ or KCl solution at $50^{\circ}C$.
(b) Give two points of differences between electrochemical and electrolytic cells.
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Q 264 Marks Questions4 Marks
Write the cell reaction and calculate the emf of the following cell at 298 K
$S n _{( s )}\left| S n ^{2+}( 0 . 0 0 4 ~ M ) \| H ^{+}( 0 . 0 2 0 ~ M )\right| H _2( g ) \overline{( 1 )} \mid P t s$ (Given : $ES _{ n }{ }^{2+} / Sn =- 0 . 1 4 V$ )
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