MCQOPTIONS
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MCQOPTIONS
This section includes 43 Mcqs, each offering curated multiple-choice questions to sharpen your Chemistry knowledge and support exam preparation. Choose a topic below to get started.
| 1. |
On passing electric current through molten aluminium chloride, 11.2 litre of \[C{{l}_{2}}\] is liberated at NTP at anode. The quantity of aluminium deposited at cathode is (at. wt. of Al = 27) [JIPMER 2002] |
| A. | 9 g |
| B. | 18 g |
| C. | 27 g |
| D. | 36 g |
| Answer» B. 18 g | |
| 2. |
How many atoms of calcium will be deposited from a solution of \[CaC{{l}_{2}}\]by a current 0.25 mA following for 60 seconds [BHU 2004] |
| A. | \[4.68\times {{10}^{18}}\] |
| B. | \[4.68\times {{10}^{15}}\] |
| C. | \[4.68\times {{10}^{12}}\] |
| D. | \[4.68\times {{10}^{9}}\] |
| Answer» B. \[4.68\times {{10}^{15}}\] | |
| 3. |
Faraday constant [KCET (Med.) 2001] |
| A. | Is a numerical constant |
| B. | Depends on equivalent |
| C. | Depends upon the current passed |
| D. | Depends on the number of electrons |
| Answer» D. Depends on the number of electrons | |
| 4. |
The aqueous solution of which of the following decomposes on passing electric current [EAMCET 1973] |
| A. | Canesugar |
| B. | Urea |
| C. | Methanol |
| D. | Potassium iodide |
| Answer» E. | |
| 5. |
From the solution of which of the following one faraday of electricity will liberate one gram atom of metal [MHCET 1999; MP PET 1993,2000; AFMC 2000] |
| A. | \[NaCl\] |
| B. | \[BaC{{l}_{2}}\] |
| C. | \[CuS{{O}_{4}}\] |
| D. | \[AlC{{l}_{3}}\] |
| Answer» B. \[BaC{{l}_{2}}\] | |
| 6. |
The value of one Faraday is [AMU 1983; AFMC 1989; MP PET 2001] |
| A. | \[95500\,\,C\,\,mo{{l}^{-1}}\] |
| B. | \[96550\,\,C\,\,mo{{l}^{-1}}\] |
| C. | \[96500\,\,C\,\,mo{{l}^{-1}}\] |
| D. | \[98500\,\,C\,\,mo{{l}^{-1}}\] |
| Answer» D. \[98500\,\,C\,\,mo{{l}^{-1}}\] | |
| 7. |
A current of strength 2.5 amp was passed through \[CuS{{O}_{4}}\] solution for 6 minutes 26 seconds. The amount of copper deposited is (Atomic weight of \[Cu=63.5\]) (1 faraday = 96500 coulombs) [EAMCET 1989; MP PET 1994] |
| A. | 0.3175 g |
| B. | 3.175 g |
| C. | 0.635 g |
| D. | 6.35 g |
| Answer» B. 3.175 g | |
| 8. |
The electric charge for electrode decomposition of one gram equivalent of a substance is[IIT 1984; KCET 1992] |
| A. | One ampere per second |
| B. | 96500 coulombs per second |
| C. | One ampere for one hour |
| D. | Charge on one mole of electrons |
| Answer» C. One ampere for one hour | |
| 9. |
How much chlorine will be liberated on passing one ampere current for 30 minutes through NaCl solution [BVP 2003] |
| A. | 0.66 mole |
| B. | 0.33 mole |
| C. | 0.66 gm |
| D. | 0.33 gm |
| Answer» D. 0.33 gm | |
| 10. |
On passing a current through \[KCl\] solution, \[19.5\,g\] of potassium is deposited. If the same quantity of electricity is passed through a solution of aluminium chloride, the amount of aluminium deposited is [EAMCET 1997] |
| A. | 4.5 g |
| B. | 9.0 g |
| C. | 13.5 g |
| D. | 27 g |
| E. | None is correct |
| Answer» B. 9.0 g | |
| 11. |
When 1 coulomb of charge is passed through electrolyte solution, then the mass deposited is equal to |
| A. | Equivalent weight |
| B. | Atomic weight |
| C. | Electrochemical equivalent |
| D. | Chemical equivalent |
| Answer» D. Chemical equivalent | |
| 12. |
On the electrolysis of aqueous solution of sodium sulphate, on cathode we get[MP PMT 1992, 2002] |
| A. | \[Na\] |
| B. | \[{{H}_{2}}\] |
| C. | \[S{{O}_{2}}\] |
| D. | \[S{{O}_{3}}\] |
| Answer» C. \[S{{O}_{2}}\] | |
| 13. |
Which of the following is not a non electrolyte [J & K 2005] |
| A. | Acetic acid |
| B. | Glucose |
| C. | Ethanol |
| D. | Urea |
| Answer» B. Glucose | |
| 14. |
Use of electrolysis is [AFMC 1995] |
| A. | Electroplating |
| B. | Electrorefining |
| C. | A and B both |
| D. | None of these |
| Answer» D. None of these | |
| 15. |
The electric conduction of a salt solution in water depends on the |
| A. | Shape of its molecules |
| B. | Size of its molecules |
| C. | Size of solvent molecules |
| D. | Extent of its ionization |
| Answer» E. | |
| 16. |
Zinc displaces copper from the solution of its salt because [MP PET 1995] |
| A. | Atomic number of zinc is more than that of copper |
| B. | Zinc salt is more soluble in water than the copper salt |
| C. | Gibbs free energy of zinc is less than that of copper |
| D. | Zinc is placed higher than copper in electro-chemical series |
| Answer» E. | |
| 17. |
Which of the following condition will increase the voltage of the cell, represented by the equation \[C{{u}_{(s)}}+2A{{g}^{+}}_{(aq)}\to C{{u}^{2+}}_{(aq)}+2A{{g}_{(s)}}\] [CBSE PMT 2001] |
| A. | Increase in the concentration of \[A{{g}^{+}}\]ion |
| B. | Increase in the concentration of \[C{{u}^{+}}\] ion |
| C. | Increase in the dimension of silver electrode |
| D. | Increase in the dimension of copper electrode |
| Answer» B. Increase in the concentration of \[C{{u}^{+}}\] ion | |
| 18. |
The standard oxidation potential of zinc and silver in water at \[298\,\,K\]are \[Zn\,\,(s)\,\,\to \,\,Z{{n}^{2+}}+2{{e}^{-}}\,;\,E=0.76\,V\] \[Ag\,\,(s)\,\,\to \,A{{g}^{2+}}+2{{e}^{-}}\,;\,E=-0.80\,V\] Which of the following reactions actually take place [NCERT 1983, 84; KCET 2003] |
| A. | \[Zn(s)+2A{{g}^{+}}(aq)\,\to \,Z{{n}^{++}}(aq)+2Ag(s)\] |
| B. | \[Z{{n}^{++}}(aq)+2Ag(s)\,\to \,2A{{g}^{+}}(aq)+Zn(s)\] |
| C. | \[Zn(s)+Ag(s)\,\to \,Z{{n}^{++}}(aq)+A{{g}^{+}}(aq)\] |
| D. | \[Z{{n}^{++}}(aq)+A{{g}^{+}}(aq)\,\to \,Zn(s)+Ag(s)\] |
| Answer» B. \[Z{{n}^{++}}(aq)+2Ag(s)\,\to \,2A{{g}^{+}}(aq)+Zn(s)\] | |
| 19. |
Nernst equation is related with |
| A. | The electrode potential and concentration of ions in the solution |
| B. | Equilibrium constant and concentration of ions |
| C. | Free energy change and E.M.F. of the cell |
| D. | None of these |
| Answer» B. Equilibrium constant and concentration of ions | |
| 20. |
Expression representing the cell potential \[(E\,\,cell)\] |
| A. | Ecathode + Eanode |
| B. | Eanode ? Ecathode |
| C. | Ecathode ? Eanode |
| D. | Eleft ? Eright |
| Answer» D. Eleft ? Eright | |
| 21. |
Standard electrode potential of \[A{{g}^{+}}/Ag\] and \[C{{u}^{+}}/Cu\] is \[+0.80V\] and \[+0.34V\] respectively. these electrodes are joint together by salt bridge if [AMU 2002] |
| A. | Copper electrode is work like cathode, then \[E_{cell}^{o}\] is \[+0.45V\] |
| B. | Silver electrode is work like anode then \[E_{cell}^{o}\] is \[-0.34V\] |
| C. | Copper electrode is work like anode then \[E_{cell}^{o}\] is \[+0.46V\] |
| D. | Silver electrode is work like cathode then \[E_{cell}^{o}\] is \[-0.34V\] |
| E. | Silver electrode is work like anode then \[E_{cell}^{o}\] will be\[+1.14V\] |
| Answer» D. Silver electrode is work like cathode then \[E_{cell}^{o}\] is \[-0.34V\] | |
| 22. |
Given standard electrode potentials \[F{{e}^{++}}+2{{e}^{-}}\,\to \,Fe\,;\,\,\,\,{{E}^{o}}=-0.440\,\,V\] \[F{{e}^{+++}}+3{{e}^{-}}\,\to \,Fe\,;\,\,\,\,{{E}^{o}}=-0.036\,\,V\] The standard electrode potential \[({{E}^{o}})\] for \[F{{e}^{+++}}+{{e}^{-}}\to \,F{{e}^{++}}\] is [AIIMS 1982] |
| A. | ? 0.476 V |
| B. | ? 0.404 V |
| C. | + 0.404 V |
| D. | + 0.771 V |
| Answer» E. | |
| 23. |
Electrode potential of \[Z{{n}^{2+}}/Zn\] is \[-0.76\,V\] and that of \[C{{u}^{2+}}/Cu\] is \[+0.34V\]. The EMF of the cell constructed between these two electrodes is [EAMCET 1992; BHU 2001; CBSE PMT 2001; KCET 1990; MHCET 1999, 2003; Pb. CET 2002; AFMC 2001;Pb. PMT 2004] |
| A. | 1.10 V |
| B. | 0.42 V |
| C. | ? 1.1V |
| D. | ? 0.42 V |
| Answer» B. 0.42 V | |
| 24. |
The standard reduction potentials at \[298\,K\]for the following half reactions are given against each \[Z{{n}^{2+}}(aq.)+2e\]⇌\[Zn(s)\];? 0.762 \[C{{r}^{3+}}(aq)+3e\]⇌\[Cr(s)\]; ? 0.740 \[2{{H}^{+}}(aq)+2e\]⇌\[{{H}_{2}}(g)\]; 0.00 \[F{{e}^{3+}}(aq)+e\]⇌\[F{{e}^{2+}}(aq)\]; 0.770 Which is the strongest reducing agent [IIT 1981; MP PET/PMT 1988; MP PMT 1989; MH CET 2001] |
| A. | \[Zn(s)\] |
| B. | \[Cr(s)\] |
| C. | \[{{H}_{2}}(g)\] |
| D. | \[F{{e}^{2+}}(aq)\] |
| Answer» B. \[Cr(s)\] | |
| 25. |
For a spontaneous reaction the \[\Delta G,\] equilibrium constant (K) and \[E_{Cell}^{o}\] will be respectively [AIEEE 2005] |
| A. | \[-ve,\,>1,\,+ve\] |
| B. | \[+ve,\,>1,\,-ve\] |
| C. | \[-ve,\,<1,\,-ve\] |
| D. | \[-ve,\,>1,\,-ve\] |
| Answer» B. \[+ve,\,>1,\,-ve\] | |
| 26. |
\[2{{H}^{+}}\,(aq)+2{{e}^{-}}\,\to \,{{H}_{2}}\,(g).\]The standard electrode potential for the above reaction is (in volts) [CPMT 1988] |
| A. | 0 |
| B. | 1 |
| C. | ? 1 |
| D. | None of these |
| Answer» B. 1 | |
| 27. |
Which one of the following reaction is not possible [MP PMT 1991] |
| A. | \[Fe+{{H}_{2}}S{{O}_{4}}\,\to \,\,FeS{{O}_{4}}+{{H}_{2}}\] |
| B. | \[Cu+2AgN{{O}_{3}}\,\to \,Cu\,{{(N{{O}_{3}})}_{2}}+2Ag\] |
| C. | \[2KBr+{{I}_{2}}\,\to \,\,2KI+B{{r}_{2}}\] |
| D. | \[CuO+{{H}_{2}}\,\to \,\,Cu+{{H}_{2}}O\] |
| Answer» D. \[CuO+{{H}_{2}}\,\to \,\,Cu+{{H}_{2}}O\] | |
| 28. |
When a copper wire is placed in a solution of \[AgN{{O}_{3}}\], the solution acquires blue colour. This is due to the formation of [Roorkee 1989] |
| A. | \[C{{u}^{2+}}\] ions |
| B. | \[C{{u}^{+}}\] ions |
| C. | Soluble complex of copper with \[AgN{{O}_{3}}\] |
| D. | \[C{{u}^{-}}\] ion by the reduction of \[Cu\] |
| Answer» B. \[C{{u}^{+}}\] ions | |
| 29. |
The \[{{E}^{0}}_{{{M}^{3+}}/{{M}^{2+}}}\]values for \[Cr,\ Mn,\ Fe\]and \[Co\]are \[-0.41,\ +1.57,\ +0.77\]and \[+1.97\ V\] respectively. For which one of these metals the change in oxidation state from \[+2\] to \[+3\]is easiest [AIEEE 2004] |
| A. | \[Fe\] |
| B. | Mn |
| C. | Cr |
| D. | Co |
| Answer» D. Co | |
| 30. |
The standard e.m.f. of a call, involving one electron change is found to be \[0.591\ V\] at 25°C. The equilibrium constant of the reaction is (\[F=96,500\ C\ mo{{l}^{-1}};\] \[R=8.314\ J{{K}^{-1}}mo{{l}^{-1}})\] [AIEEE 2004] |
| A. | \[1.0\times {{10}^{10}}\] |
| B. | \[1.0\times {{10}^{5}}\] |
| C. | \[1.0\times {{10}^{1}}\] |
| D. | \[1.0\times {{10}^{30}}\] |
| Answer» B. \[1.0\times {{10}^{5}}\] | |
| 31. |
Which of the following is the most electropositive element [Pb. PMT 2000] |
| A. | Carbon |
| B. | Calcium |
| C. | Chlorine |
| D. | Potassium |
| Answer» E. | |
| 32. |
Which of the following is a highly corrosive salt [AFMC 2005] |
| A. | \[FeC{{l}_{2}}\] |
| B. | \[PbC{{l}_{2}}\] |
| C. | \[H{{g}_{2}}C{{l}_{2}}\] |
| D. | \[HgC{{l}_{2}}\] |
| Answer» E. | |
| 33. |
If X is the specific resistance of the solution and M is the molarity of the solution, the molar conductivity of the solution is given by [Kurukshetra CEE 2002] |
| A. | \[\frac{1000X}{M}\] |
| B. | \[\frac{1000}{MX}\] |
| C. | \[\frac{1000M}{X}\] |
| D. | \[\frac{MX}{1000}\] |
| Answer» C. \[\frac{1000M}{X}\] | |
| 34. |
Which of the following statements is not applicable to electrolytic conductors [AIIMS 1991] |
| A. | New products show up at the electrodes |
| B. | Ions are responsible for carrying the current |
| C. | Show a positive temperature coefficient for conductance |
| D. | A single stream of electrons flows from cathode to anode |
| Answer» E. | |
| 35. |
Which one of the following statements is correct [MP PET 1997] |
| A. | The oxidation number of oxygen in \[K{{O}_{2}}\] is zero |
| B. | The specific conductance of an electrolyte solution decreases with increase in dilution |
| C. | \[S{{n}^{2+}}\] oxidises \[F{{e}^{3+}}\] |
| D. | \[Zn/ZnS{{O}_{4}}\] is a reference electrode |
| Answer» E. | |
| 36. |
When lead storage battery is charged [MP PET 2003] |
| A. | \[Pb{{O}_{2}}\]is dissolved |
| B. | \[{{H}_{2}}S{{O}_{4}}\]is regenerated |
| C. | \[PbS{{O}_{4}}\]is deposited on lead electrode |
| D. | Lead is deposited on lead electrode |
| Answer» D. Lead is deposited on lead electrode | |
| 37. |
Which of the following statement is true for the electrochemical Daniel cell [AIIMS 2004] |
| A. | Electrons flow from copper electrode to zinc electrode |
| B. | Current flows from zinc electrode to copper electrode |
| C. | Cations move toward copper electrode which is cathode |
| D. | Cations move toward zinc electrode |
| Answer» D. Cations move toward zinc electrode | |
| 38. |
In the cell \[Zn\,\,|\,\,Z{{n}^{2+}}\,\,||\,\,C{{u}^{2+}}\,\,|\,\,Cu,\] the negative electrode is [MP PMT 1995] |
| A. | \[Cu\] |
| B. | \[C{{u}^{2+}}\] |
| C. | \[Zn\] |
| D. | \[Z{{n}^{2+}}\] |
| Answer» D. \[Z{{n}^{2+}}\] | |
| 39. |
In electrolysis of dilute \[{{H}_{2}}S{{O}_{4}}\]using platinum electrodes [DPMT 1983; IIT 1983; Kurukshetra CET 2002; AFMC 2005] |
| A. | \[{{H}_{2}}\] is evolved at cathode |
| B. | \[N{{H}_{3}}\] is produced at anode |
| C. | \[C{{l}_{2}}\] is obtained at cathode |
| D. | \[{{O}_{2}}\] is produced |
| Answer» B. \[N{{H}_{3}}\] is produced at anode | |
| 40. |
Mark the false statement[MP PET 1997] |
| A. | A salt bridge is used to eliminate liquid junction potential |
| B. | The Gibbs free energy change, \[\Delta G\] is related with electromotive force \[(E)\], as \[\Delta G=-nFE\] |
| C. | Nernst equation for single electrode potential is \[E={{E}^{o}}-\frac{RT}{nF}\,\ln \,{{a}_{{{M}^{n+}}}}\] |
| D. | The efficiency of a hydrogen oxygen fuel cell is 23% |
| Answer» E. | |
| 41. |
The specific conductance of a solution is 0.2 \[oh{{m}^{-1}}c{{m}^{-1}}\]and conductivity is 0.04 \[oh{{m}^{-1}}\]. The cell constant would be [RPET 1999] |
| A. | 1 \[c{{m}^{-1}}\] |
| B. | 0 \[c{{m}^{-1}}\] |
| C. | 5 \[c{{m}^{-1}}\] |
| D. | 0.2 \[c{{m}^{-1}}\] |
| Answer» D. 0.2 \[c{{m}^{-1}}\] | |
| 42. |
If the conductance and specific conductance of a solution is one then its cell constant would be [RPET 1999] |
| A. | 1 |
| B. | Zero |
| C. | 0.5 |
| D. | 4 |
| Answer» B. Zero | |
| 43. |
Which of the substances \[Na,\,\,Hg,\,\,S,\,\,Pt\] and graphite can be used as electrodes in electrolytic cells having aqueous solutions [AIIMS 1982] |
| A. | \[Na,\,\,Pt\]and graphite |
| B. | \[Na\]and \[Hg\] |
| C. | \[Pt\]and graphite only |
| D. | \[Na\]and \[Al\]only |
| Answer» D. \[Na\]and \[Al\]only | |