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Electrochemistry Test - 4
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Electrochemistry Test - 4
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  • Question 1/15
    1 / -0.25

     

    Emf of the cell  

    Mg (s) | Mg2+  (0.001M) || Cu2+ (0.0001M) | Cu(s)  at 298 K is

     

    Solutions

     

     

     

     

  • Question 2/15
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    Emf of the cell  

    Fe (s) | Fe2+  (0.001 M)|| H+ (1M)|H2  (g) (1 bar) |Pt(s)  at 298 K is

    (Given: Eocell   ​= +0.44  V)

     

    Solutions

     

     

    ⇒Ecell   ​= 0.44 + 0.089V

    ⇒Ecell ​= 0.53V

     

     

  • Question 3/15
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    The conductivity of 0.20 M solution of KCl at 298 K is 0.0248 S  cm-1 . Calculate its molar conductivity. 

     

    Solutions

     

     

    k  (Conductivity) =0.0248  Scm−1 , C (molarity) = 0.20  M, T  (temperature) = 298  K
    Λm ​= ? (molar conductivity) 

    Λm ​= (1000 ×k ​) / C = (1000 ×0.0248) / 0.20 ​= 124  S  cm2  mol−1

    The molar conductivity is  124  S  cm2  mol−1

     

     

  • Question 4/15
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    The resistance of a conductivity cell containing 0.001M KCl solution at 298 K is 1500 Ω. What is the cell constant if conductivity of 0.001M KCl solution at 298 K is 0.146 ×10-3  S cm-1 .

     

    Solutions

     

     

    Κ= G x cell constant and G = 1/R.

     

     

  • Question 5/15
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    How much charge is required for the reduction of 1 mol of Al3+  to Al?

     

    Solutions

     

     

    For reduction of 1 mol of  Al3+  to Al, 3 mol of electrons are required so total charge will be 3F.

     

     

  • Question 6/15
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    How much electricity in terms of Faraday is required to produce 40.0 g of Al from molten  Al 2O3 ?

     

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  • Question 7/15
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    Three electrolytic cells A, B, C containing solutions of ZnSO4 , AgNO3 and CuSO4 , respectively are connected in series. A steady current of 1.5 amperes was passed through them until 1.45 g of silver deposited at the cathode of cell. How long did the current flow? What mass of copper and zinc were deposited?  

     

    Solutions

     

     

    And mass of Zn and Cu deposited will be in ratio of their equivalent mass.

     

     

  • Question 8/15
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    The standard emf of galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the reaction of the cell is

     

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  • Question 9/15
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    An increase in equivalent conductance of a strong electrolyte with dilution is mainly due to

     

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    Equivalent conductance increases on dilution for a strong electrolyte because of increase in mobility of ions.

     

     

  • Question 10/15
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    For the reduction of silver ions with copper metal the standard cell potential was found to be +0.46V at 25 °C. The value of standard Gibbs energy, ΔG °wll be (F = 96500 C mol-1 )

     

    Solutions

     

     

     

     

  • Question 11/15
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    Which of the following electrolytic solutions has the least specific conductance?

     

    Solutions

     

     

    Specific conductance decreases with dilution because of decrease in the number of ions per unit volume.

     

     

  • Question 12/15
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    The highest electrical conductivity of the following aqueous solutions is of

     

    Solutions

     

     

    Acidity increases on attaching electron withdrawing group because of stability of conjugate base.

     

     

  • Question 13/15
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    The standard electrode potential is measured by

     

    Solutions

     

     

    Voltmeter measures the potential.

     

     

  • Question 14/15
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    When KMnO4 acts as an oxidizing agent and ultimately forms MnO42- , MnO2 , Mn2 O3 , and Mn2+  then the number of electrons transferred in each case 

     

    Solutions

     

     

    No. of electrons = change in oxidation number of active elemnt.

     

     

  • Question 15/15
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    On the basis of the following E °values, the strongest oxidizing agent is: 

     

    Solutions

     

     

    • The strongest oxidizing agent is one having more positive or less negative reduction potential.
    • For the strongest oxidizing agent, the oxidizing potential should be the least.

    Here, the oxidizing potential of  Fe+2  is less than that of  [Fe(CN)6 ​]4 − . Therefore, Fe+2  is a stronger oxidizing agent than  [Fe(CN)6 ​]4 − .

    • Also, the stronger oxidizing agent should easily reduce itself.

    Here, Fe+3  is easily reduced than  Fe+2 . Therefore, among all the four, Fe+3  is the stronger oxidizing agent.

     

     

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