Q.1
Measuring Zeta potential is useful in determining which property of colloidal solution? [NEET 2020]
  • a) Stability of the colloidal particles
  • b) Size of the colloidal particles
  • c)Viscosity
  • d)OSolubility
Q.2
On electrolysis of dil. sulphuric acid using Platinum (Pt) electrode, the product obtained at anode will be ... [NEET 2020]
  • a) H2S gas
  • b) SO2 gas
  • c) Hydrogen gas
  • d) Oxygen gas
Q.3
The number of Faradays(F) required to produce 20 g of calcium from molten CaCl2 (Atomic mass of Ca = 40 g mol-1) is [NEET 2019]
  • a) 3
  • b) 4
  • c) 1
  • d) 2
Q.4
What is the change in oxidation number of carbon in the following reaction? CH4 (g) + 4Cl2 (g) → CClsub>4 (l)+ 4HCl(g) [NEET 2019] Answer: (a)
  • a) – 4 to + 4
  • b) 0 to – 4
  • c) + 4 to + 4
  • d) 0 to + 4
Q.5
Which of the following reactions are disproportionation reaction? [NEET 2019] (a) 2Cu+ → Cu2+ + Cu0 (b) 3MnO42- + 4H+ → 2MnO4 + MnO2 + 2H2O (c) 2KMnO4 → K2 MnO4+ MnO2 + O2 (d) 2MnO4- + 3Mn2+ + 2H2 O +5MnO2+ 4H+ Select the correct option from the following
  • a)(a) and (b) only
  • b) (a), (b) and (c)
  • c)(a), (c) and (d)
  • d) (a) and (d) only
Q.6
For the cell reaction 2Fe3+ (aq) + 2I- (aq) → 2Fe2+ (aq) + I2 (aq) EΘcell=0.24 V at 298 K. The standard Gibbs energy (ΔrG Θ) of the cell reaction is : [Given that Faraday constant F = 96500 C mol-1]
  • a) – 46.32 kJ mol–1
  • b) – 23.16 kJ mol–1
  • c)46.32 kJ mol–1
  • d)23.16 kJ mol–1
Q.7
he correct order of N-compounds in its decreasing order of oxidation states is ... [NEET 2018]
  • a) HNO3, NH4Cl, NO, N2 2mole -1
  • b)HNO3, NO, NH4Cl, N2
  • c)HNO3, NO, N2, NH4Cl
  • d) NH4Cl, N2, NO, HNO3
Q.8
Consider the change in oxidation state of Bromine corresponding to different emf values as shown in the diagram below : Then the species undergoing disproportionation is [NEET 2018]
ch-7_que_no-8_img_no1.png
  • a) Br2
  • b) BrO4-
  • c) 3BrO3-
  • d) HBrO
Q.9
For the redox reaction ... [2018] MnO4- + C2O42- + H+ → Mn2+ + CO2 + H2O the correct coefficients of the reactants for the balanced equation are
  • a)MnO4- = 3; C2O42- = 16; H+ = 5
  • b) MnO4- = 2; C2O42- = 5; H+ = 16
  • c) MnO4- = 16; C2O42- = 5; H+ = 2
  • d) MnO4- = 5; C2O42- = 16; H+ = 2
Q.10
For a cell involving one electron E&dgecell = 0.59 V at 298 K, the equilibrium constant for the cell reaction is : Given that
ch-7_que_no-10_img_no1.png
  • a) 1.0 × 102
  • b) 1.0 × 105
  • c) 1.0 × 1010
  • d) 1.0 × 1030
Q.11
The chemical reaction.2AgCls + H2(g) → 2HCl(aq) + 2Ag(s)taking place in a galvanic cell is represented by the notation [ AFMC 2009]
  • a)Pts| H2(g).1 bar| 1 M KCl(aq)| AgCl(s)| Ag(s)
  • b)Pts| H2(g).1 bar| 1 M HCl(aq)| 1M Ag+(aq)| Ag(s)
  • c)Pts| H2(g).1 bar| 1 M HCl(aq)| AgCl(s)| Ag(s)
  • d)Pts| H2(g).1 bar| 1 M HCl(aq)| Ag(s)| AgCl(s)
Q.12
Among the following compound, the oxidation state of Mn is highest in ..[ AFMC 2010]
  • a) KMnO4
  • b) K2MnO4
  • c) MnO2
  • d) Mn2O3
Q.13
In alkaline condition KMhO0 reacts as follows: 2KMnO4 + 2KOH → 2K2MnO4 + H2O + O The equivalent weight of KMnO4 would be ( At. mass of K=39, Mn=55, O=16)
  • a)79.0
  • b) 31.6
  • c)52.7
  • d)158.0
Q.14
How many electrons are involved in oxidation by KMnO4 in basic medium
  • a) 1
  • b) 2
  • c)5
  • d)3
Q.15
Which of the following chemical reactions depicts the oxidising behavior of H2SO4 [ AIEEE 2006]
  • a) 2HI + H2SO4 → I2 + SO2 + 2H2O
  • b)Ca(OH)2 + H2SO4 → CaSO4 + 2H2O
  • c)NaCl + H2SO4 → NaHSO4 + HCl
  • d)2PCl5 + H2SO4 → 2POCl3 +2HCl + SO2Cl2
Q.16
The reaction 3ClO- → Cl3- + 2Cl- is an example of ..[ IIT 2001]
  • a) Oxidation reaction
  • b) Reduction reaction
  • c) disproportion reaction
  • d) decomposition reaction
Q.17
Cr2O72- + X + H+ → Cr3+ + H2O + oxidised product of X X in above reaction can not be
  • a)C2O42-
  • b)SO42-
  • c)S2-
  • d)Fe2+
Q.18
Which one of the following leads to redox reaction
  • a) AgNO3 + HCl
  • b) KOH + HCl
  • c)KI + Cl2
  • d)NH3 + HCl
Q.19
On reduction of KMnO4 by oxalic acid in acidic medium, the oxidation number of Mn changes. What is the magnitude of this charge? [ AIEEE 2007]
  • a) From 7 to 2
  • b) From 6 to 2
  • c)From 5 to 2
  • d)From 7 to 4
Q.20
Number of moles of K2Cr2O7 reduced by one mole of Sn2+ ions is [ Hariyana CEET 2000]
  • a) 1/3
  • b) 3
  • c) 1/6
  • d) 6
Q.21
In which of the following changes there is a transfer of five electrons?
  • a)MnO4- → Mn2+
  • b) CrO4- → Cr3+
  • c)MnO4- → MnO2
  • d)Cr2O72- → 2Cr3+
Q.22
he colour of K2Cr2O7 changes from red orange to lemon yell on treatment with aqueous KOH because of
  • a) Reduction of Cr(VI) to Cr(III)
  • b) Formation of chromium ion to chromate
  • c)Conversion of dichromate ion to chromate
  • d)Oxidation of potassium hydroxide to potassium peroxide
Q.23
Cr2O72- → Cr3+ eq.wt of Cr2O72- is
  • a)mol.wt/6
  • b) mol.wt/3
  • c)mol.wt./4
  • d)mol.wt./8
Q.24
What is the equivalent mass of IO4- when it is converted into I2 in acid medium
  • a) M/6
  • b) M/7
  • c) M/5
  • d) M/4
Q.25
xMnO4-+ yHSO3- → 2Mn2+ + 2H2O + OH-+ zSO42- In this reaction value of x, y and z are
  • a)2, 5, 5
  • b) 5, 2, 9
  • c)3, 5, 5
  • d)2, 6, 6
Q.26
The standard reduction potential of Cu2+ / Cu and Cu2+ / Cu+ are 0.337 and 0.153 respectively. the standard electrode potential of Cu+ / Cu half cell is ... [ IIT 1997]
  • a) 0.184 V
  • b) 0.827 V
  • c)0.521 V
  • d)0.490 v
Q.27
A current of 2amp when passed for 5 hours through a moltan salt deposits 22.2 g of metal of atomic massThe oxidation state of the metal in the metal salt is
  • a) +1
  • b) +2
  • c) +3
  • d) +4
Q.28
The compound that can work both as an oxidising as well as a reducing agent is [ CPMT 1986]
  • a) KMnO4
  • b) H2O2
  • c) Fe2(SO4)3
  • d) K2Cr2O7
Q.29
For the redox reaction. the correct coefficient of the reactants for the balanced reaction are
ch-7_que_no-26_img_no1.png
  • a) MnO4-=2; C2O4-=5; H+=16
  • b) MnO4-=16; C2O4-=3; H+=12
  • c)MnO4-=15; C2O4-=16; H+=12
  • d)MnO4-=2; C2O4-=16; H+=5
Q.30
In acidic, dichromatic ion oxides ferrous ion to ferric ion. If the gram molecular weight of potassium dichromate is 294 grams, its gram equivalent weight is ... grams
  • a) 294
  • b) 127
  • c)49
  • d)24.5
0 h : 0 m : 1 s