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An example of a disproportionation reaction is :

  • Option 1)

    2CuBr\rightarrow Cubr_{2}+Cu

  • Option 2)

    2KMnO_{4}\rightarrow K_{2}MnO_{4}+MnO_{2}+O_{2}

  • Option 3)

    2MnO^{-}_{4}+10I^{-}+16H^{+}\rightarrow 2Mn^{2+}+5I_{2}+8H_{2}O

  • Option 4)

    2NaBr+CI_{2}\rightarrow 2NaCI+Br_{2}

  Disproportionation Reactions - A special type of redox reaction in which one oxidation state is simultaneously oxidised and reduced. One of the reacting substances in a disproportionation reaction always contains an element that can exist in at least three oxidation states.  - wherein +1     -1                     +1    -2               0       Disproportionation reactions are those where...

Consider the statements S1 and S2 :

S1 : Conductivity always increases with decrease in the concentration of electrolyte.

S2 : Molar conductivity always increases with decrease in the concentration of electrolyte.

The correct option among the following is : 

  • Option 1)

    Both S1 and S2 are wrong

  • Option 2)

    S1 is wrong and S2 is correct

  • Option 3)

    Both S1 and S2 are correct

  • Option 4)

    S1 is correct and S2 is wrong

Molar conductivity is given as   , K = conductivity & c = concentration We know that  Conductivity increases with increase in concentration.  Molar Conductivity increases with decrease in concentration.  S1 is wrong & S2 is correct.  option (2) is correct.Option 1)Both S1 and S2 are wrongOption 2)S1 is wrong and S2 is correctOption 3)Both S1 and S2 are correctOption 4)S1 is correct and S2 is wrong

ven : 

Co^{3+}+ e^{-}\rightarrow Co^{2+}+;E^{0}=+1.81V

Pb^{4+}+2 e^{-}\rightarrow Pb{2+}+;E^{0}=+1.67V

Ce^{4+}+ e^{-}\rightarrow Ce{3+}+;E^{0}=+1.61V

Bi ^{3+}+ 3e^{-}\rightarrow Bi;E^{0}=+0.20 V

Oxidising power of the species will increase in the  order: 

 

  • Option 1)

    Bi^{3+}< Ce^{4+}< Pb^{4+}< Co^{3+}

  • Option 2)

    Ce^{4+}< Pb^{4+}< Bi^{3+}< Co^{3+}

  • Option 3)

    Co^{3+}< Ce^{4+}< Bi^{3+}< Pb^{4+}

  • Option 4)

    Co^{3+}< Pb^{4+}< Ce^{4+}< Bi^{3+}

 
  Electrode Potential - The potential associated with each electrode is known as electrode potential. -     Electro-chemical series - The standard reduction potential of a large number of electrodes have been measured using standard hydrogen electrode as the reference electrode. These various electrode can be arranged in increasing electrode potential. -       Standard Electrode Potential Value...

Which one of the following graphs between molar conductivity \left ( \wedge _{m} \right ) versus \sqrt{C} is correct ?

  • Option 1)

  • Option 2)

  • Option 3)

      

  • Option 4)

     

        electrolyte have higher value of   w..r.t   because  ionise more hydrated w.r.t  ion Option 1)Option 2)Option 3)  Option 4) 

A solution of Ni(NO_{3})_{2} is electrolysed between platinium electrodes using 0.1 faraday electricity . How many mole of Ni will be deposited at the cathode ?

  • Option 1)

    0.05

  • Option 2)

    0.20

  • Option 3)

    0.15

  • Option 4)

    0.10

  Faraday's first law of electrolysis - The mass of any substance deposited or dissolved at any electrode during electrolysis is directly propotional to the quantity of electricity passed through the solution. - wherein W = Z I t Z = mass of electrolyte get deposited Z = electro chemical equivalent                need 2 mole of   for 1 mole of   Option 1) Option 2) Option 3) Option 4)

The standard Gibbs energy for the given cell reaction in KJ\; mol^{-1} at 298\; K is :

Zn\left ( s \right )+Cu^{2+}\left ( aq \right )\rightarrow Zn^{2+}\left ( aq \right )+Cu\left ( s \right ),

E^{0}=2\; V\; at\; 298\; K

(Faraday's constant, F=96000\; C\; mol^{-1})

  • Option 1)

     - 384

  • Option 2)

     384

  • Option 3)

    192

  • Option 4)

    -192

 
We know,                                                         Option 1)   Option 2)   Option 3) Option 4)

The correct order of the oxidation states of nitrogen in NO,N_{2}O,NO_{2} and N_{2}O_{3} is :

  • Option 1)

     NO_{2}< NO< N_{2}O_{3}< N_{2}O

  • Option 2)

     NO_{2}< N_{2}O_{3}< NO< N_{2}O

     

     

  • Option 3)

     N_{2}O< N_{2}O_{3}< NO< NO_{2}

  • Option 4)

    N_{2}O<NO< N_{2}O_{3}< NO_{2}

Option 4

 

Calculate the standard cell potential (in V) of the cell in which following reaction takes place:

Fe^{2+}\left ( aq \right )+Ag^{+}\left ( aq \right )\rightarrow Fe^{3+}\left ( aq \right )+Ag\left ( s \right )

Given that

E_{Ag^{+}/Ag}^{0}=xV

E_{Fe^{2+}/Fe}^{0}=yV

E_{Fe^{3+}/Fe}^{0}=zV

  • Option 1)

    x-z

  • Option 2)

    x-y

  • Option 3)

    x+2y-3z

  • Option 4)

    x+y-z

                                          Given              Cell equation :-                             (Oxidation)                    (Cathode Reduction)  Std. EMF of given cell reaction:-              (iii-ii)     Put this in eqn (i)  Option 1)x-zOption 2)x-yOption 3)x+2y-3zOption 4)x+y-z

Given that E_{O_{2}/H_{2}O}^{\circleddash}=+1.23V;

E_{S_{2}O_{8}^{2-}/SO_{4}^{2-}}^{\circleddash}=2.05V;

E_{Br_{2}/Br^{-}}^{\circleddash}=+1.09 \; V;

E_{Au^{3+}/Au}^{\circleddash}=+1.4\; V;

The strongest oxidizing agent is :

  • Option 1)

    O_{2}

  • Option 2)

    Br_{2}

  • Option 3)

    S_{2}O_{8}^{2-}

     

  • Option 4)

    Au^{3+}

For strongest oxidising agent, standard reduction potential should be highest and so, it is highest for .  Option 1)Option 2)Option 3)  Option 4)
 Potassium permanganate is an inorganic chemical compound with the formula KMnO4. It is a salt consisting of K+ and MnO4 − ions.It known as permanganate of potash, it is a strong oxidizing agent. It dissolves in water to give intensely purple solutions.
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different electrons we use dg =-nfe
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The Standard E0 value of half cell Fe Fe2 is:

Consider the following standard electrode potentials (E0 in volts) in aqueous solution :

Based on these data, which of the following statements is correct ?

  • Option 1)

    Tl+ is more stable than Al3+

  • Option 2)

    Al+ is more stable than Al3+

  • Option 3)

     Tl+ is more stable than Al+

  • Option 4)

    Tl3+ is more stable than Al3+

     

 
Option 1) Tl+ is more stable than Al3+ Option 2) Al+ is more stable than Al3+ Option 3)  Tl+ is more stable than Al+ Option 4) Tl3+ is more stable than Al3+  
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For the cell Zn(s)\left | Zn^{2+}(aq) \right |\left | M^{x+}(aq) \right |M(s), different half cells and their standerd electrode potential are given below :

If E^{0}_{zn^{2+}/zn} = -0.76V ,which cathode will give a maximun value of E^{0}_{cell}  per electron transfered?

  • Option 1)

    Au^{3+}/Au

  • Option 2)

    Fe^{3+}/Fe^{2+}

  • Option 3)

    Fe^{2+}/Fe

  • Option 4)

    Ag^{+}/Ag

  Standard Electrode Potential Value - As we know that E0cell is maximum with E0Au+3/Au(s) among others In thecell reaction elecrons transfered quantity doesn't matter. -    Option 1)Option 2)Option 3)Option 4)

 Given : 

(i) C (graphite)+ O_{2}(g)\rightarrow CO_{2}(g);\\\Delta rH^{\Theta }=x\: kJ mol^{-1}

(ii) C (graphite)+\frac{1}{2} O_{2}(g)\rightarrow CO_{2}(g);\\\Delta rH^{\Theta }=y \: \: kJ mol^{-1}

(iii) CO(g)+\frac{1}{2} O_{2}(g)\rightarrow CO_{2}(g);\\\Delta rH^{\Theta }= z\: kJ mol^{-1}

Based on the above thermochemical equations, find out which one of the following algebraic relationships is correct ?

  • Option 1)

    y = 2z - x

  • Option 2)

    x= y - z

  • Option 3)

    z = x+y

  • Option 4)

    x = y + z

  Electrochemistry - It is the study of production of electricity from energy released during spontaneous chemical reactions and the use of electrical energy to bring about non spontaneous chemical transformations. Balancing of Redox Reactions - Oxidation number method - wherein 1. Write the correct formula for each reactant and product. 2. Identify atom whose oxidation number is changed. 3....

In the reaction of oxalate with permannganate in acidic medium, the number of electrons involved in producing one molecule of CO_{2} is:

  • Option 1)

    10

  • Option 2)

    2

  • Option 3)

    1

  • Option 4)

    5

  Balancing of Redox Reactions - Oxidation number method - wherein 1. Write the correct formula for each reactant and product. 2. Identify atom whose oxidation number is changed. 3. Calculate increase / decrease in oxidation number per atom and for the entire molecule / ion in which it occures. 4. Add  on appropriate side so that the total ionic charges of reactants and products are equal. 5....

In the cell

Pt_{\left ( s \right )}\mid H_{2}\left ( g, 1 bar \right )\mid HCl_{\left ( aq \right )}\mid AgCl_{\left ( s \right )}\mid Pt_{\left ( s \right )} the cell potential is 0.92V when a 10-6 molal HCl solution is used . The stansard electrode potential of \left ( AgCl/ag,Cl^{-} \right ) electrode is:\left \{ Given \frac{2.303RT}{F}=0.06 V \, at 289 K \right \}

  • Option 1)

    0.20 V

  • Option 2)

    0.40V

  • Option 3)

    0.76V

  • Option 4)

    0.94V

  Nernst Equation - - wherein is concentration of species F= 96487 C  R= 8.314  T= Temperature in kelvin   As we learned in cell potential At Anode : At Cathode : = 0.2 V  Option 1)0.20 VOption 2)0.40VOption 3)0.76VOption 4)0.94V

Consider the following reduction processes

The reducing power of the metals increases in order :

 

  • Option 1)

     

    Ca < Zn < Mg < Ni

  • Option 2)

     

    Ni < Zn < Mg < Ca

  • Option 3)

     

    Zn < Mg < Ni < Ca

  • Option 4)

     

    Ca < Mg < Zn < Ni

  Reduction - Removal of Oxygen / electronegative element from a substance of addition of hydrogen / electropositive element to substance. - wherein e.g.       Electrode Potential - The potential associated with each electrode is known as electrode potential. -     Standard Electrode Potential Value - -     Standard reduction potential - It measure the tendency of a chemical species to acquire...
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