Which element exhibits both positive and negative oxidation states?

  • Cs

  • Ne

  • I

  • F

The balanced equation for the reaction between chlorine and sulphur dioxide in water is-

  • Cl2(s) + SO2(aq) + 2H2O(I) →2Cl-(aq) + SO42-(aq) + 4H+(aq)

  • 3Cl2(s) + SO2(aq) + 2H2O(I) →Cl-(aq) + SO42-(aq) + 3H+(aq)

  • Cl2(s) + 3SO2(aq) + H2O(I) →Cl-(aq) + 2SO42-(aq) + 4H+(aq)

  • 2Cl2(s) + SO2(aq) + H2O(I) →2Cl-(aq) + SO42-(aq) + 4H+(aq)

The set of metals that can show disproportionation reaction is -

  • Cu, Na, Li

  • Mg, F, Ne

  • P, Cl, S

  • Mn, Cu, Ga

The maximum weight of nitric oxide that can be obtained starting only with 10.00 g of ammonia and 20.00 g of oxygen is -

  • 9 g

  • 15 g

  • 12 g

  • 11g

In Fe0.90O , Fe is present in +2 and +3 oxidation state. What is the mole fraction  of Fe3+ in the compound ? 

  • 0.22

  • 0.77

  • 0.90

  • None

The correct decreasing order of following metals in which they displace each other from the solution of their salts is: 
           Al, Cu, Fe, Mg and Zn.

1) Al> Zn > Fe > Cu > Mg

2) Zn > Fe > Cu > Mg > Al

3) Mg > Al > Zn > Fe > Cu

4) Fe > Mg > Zn > Al > Cu

  • 1
  • 2
  • 3
  • 4

The correct statement about the electrolysis of an aqueous solution of AgNO3 with Ag electrode is-

  •  Ag+ion gets oxidised at cathode; Ag(s) is reduced at anode

  •  H2O gets reduced at cathode; H2O gets oxidised at anode

  • Ag+ion gets reduced at cathode; H2O gets oxidised at anode

  •  Ag+ion gets reduced at cathode; Ag(s) gets oxidised at anode

The reactions of electrolysis for a dilute solution of H2SO4 with platinum electrode are-

  •  H+ ion reduce at cathode; H2O oxidised at anode

  •  H+ ion reduce at cathode; SO42- ion oxidised at anode

  •  H2O ion reduce at cathode; H2O oxidised at anode

  •  H2O ion reduce at cathode; H+ ion oxidised at anode

The correct statement about electrolysis of an aqueous solution of CuCl2 with Pt electrode is-

  •  Cu2+ ion reduced at the cathode; Cl- ion oxidized at the anode 

  •  Cu2+ ion reduced at the anode; Cl- ion oxidized at the cathode

  •  Cu2+ ion reduced at the cathode; H2O ion oxidized at the anode 

  •  H2O ion reduced at the cathode; Cl- ion oxidized at the anode 

The oxidizing agent and reducing agent in the given reaction are

3N2H4l+4ClO3aq-6NOg+4Claq-+6H2Ol

  •  Oxidising agent = N2H4; Reducing agent = ClO3-

  •  Oxidising agent = ClO3-; Reducing agent = N2H4

  •  Oxidising agent = N2H4 ; Reducing agent = N2H4

  •  Oxidising agent = ClO3- ; Reducing agent = ClO3-

The oxidising agent and reducing agent in the given reaction are

Cl2O7g+4H2O2aq+2OHaq-2ClO2aq-+4O2g+5H2Ol

  •  Oxidizing agent = H2O2; Reducing agent = Cl2O7

  •  Oxidizing agent = Cl2O7; Reducing agent = H2O2

  •  Oxidizing agent = H2O2; Reducing agent = H2O2

  • None of the above

Given a galvanic cell with the following reaction

Zn(s)  + 2Ag+(aq) Zn+2(aq) + Ag(s) 

The negatively charged electrode will be-

  • Zn

  • Ag

  • Both

  • None of  the above

The oxidation states of the central atom in the given species are, respectively:

H4P2O7  and H2S2O7

  • 0 and +6

  • +3 and +4

  • +4 and +2

  • +5 and +6

KI3 , H2S4O6

The oxidation numbers of iodine and sulphur in the above compounds are, respectively?

 1. 13; 42. 2.5; 133. 13; 2.54. 2.5; 3

  • 1
  • 2
  • 3
  • 4

The metal displacement reaction among the following is -

  •  Fe+2HClFeCl2+H2

  •  2Pb(NO3)22PbO+4NO2+O2

  •  2KClO32KCl+3O2

  •  Cr2O3+2AlAl2O3+2Cr

2 Na(s) + H2(g)  2 NaH (s)
The incorrect statement among the following regarding above mentioned reaction is-

  • Na gets oxidised
  • It is a redox reaction
  • NaH is an ionic hydride
  • None of the above

2Cu2O(s) + Cu2S(s) → 6Cu(s) + SO2(g)
The correct statement among the following regarding above mentioned reaction is-

  • Cu is reduced and Cu(I) is an reductant
  • Sulphur is reduced and S in Cu2S acts as oxidant
  • Cu(I) is an oxidant and Cu(I) is reduced.
  • Sulphur is reduced and Cu is oxidised

The species among the following that does not show a disproportionation reaction is-

ClO, ClO2\(ClO_{3}^{-}\) and ClO4

  • ClO

  • ClO2
  • ClO4
  • \(ClO_{3}^{-}\)

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