MCQOPTIONS
Saved Bookmarks
MCQOPTIONS
This section includes 11242 Mcqs, each offering curated multiple-choice questions to sharpen your Joint Entrance Exam - Main (JEE Main) knowledge and support exam preparation. Choose a topic below to get started.
| 6001. |
During the process of electrolytic refining of copper, some metals present as impurity settle as 'anode mud'. These are [AIEEE 2005] |
| A. | Sn and Ag |
| B. | Pb and Zn |
| C. | Ag and Au |
| D. | Fe and Ni |
| Answer» D. Fe and Ni | |
| 6002. |
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 | |
| 6003. |
What weight of copper will be deposited by passing 2 Faradays of electricity through a cupric salt (Atomic weight of Cu = 63.5) [NCERT 1975; CPMT 1977, 79] |
| A. | 2.0 gm |
| B. | 3.175 gm |
| C. | 63.5 gm |
| D. | 127.0 gm |
| Answer» D. 127.0 gm | |
| 6004. |
The number of coulombs required to reduce 12.3 g of nitrobenzene to aniline [UPSEAT 2003] |
| A. | 115800 C |
| B. | 5790 C |
| C. | 28950 C |
| D. | 57900 C |
| Answer» E. | |
| 6005. |
The law of electrolysis were proposed by [CPMT 1982;Pb.CET 2003] |
| A. | Kohlraush |
| B. | Faraday |
| C. | Nernst |
| D. | Berthelot |
| Answer» C. Nernst | |
| 6006. |
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. \[4.68\times {{10}^{15}}\] | |
| 6007. |
An electric current is passed through silver nitrate solution using silver electrodes. 10.79 g of silver was found to be deposited on the cathode if the same amount of electricity is passed through copper sulphate solution using copper electrodes, the weight of copper deposited on the cathode is [Kerala PMT 2004] |
| A. | 6.4 g |
| B. | 2.3 g |
| C. | 12.8 g |
| D. | 1.6 g |
| E. | 3.2 g |
| Answer» F. | |
| 6008. |
In a galvanic cell, the electrons flow from [KCET 2004] |
| A. | Anode to cathode through the solution |
| B. | Cathode to anode through the solution |
| C. | Anode to cathode through the external circuit |
| D. | Cathode to anode through the external circuit |
| Answer» D. Cathode to anode through the external circuit | |
| 6009. |
In the electrolysis of water, one Faraday of electrical energy would evolve [DCE 2004] |
| A. | One mole of oxygen |
| B. | One g atom of oxygen |
| C. | 8 g of oxygen |
| D. | 22.4 litres of oxygen |
| Answer» D. 22.4 litres of oxygen | |
| 6010. |
4 g of copper was dissolved in concentrated nitric acid. The copper nitrate solution on strong heating gave 5 g of its oxide. The equivalent weight of copper is [KCET 2004] |
| A. | 23 |
| B. | 32 |
| C. | 12 |
| D. | 20 |
| Answer» C. 12 | |
| 6011. |
When 1F of electricity is passed through acidulated water, \[{{O}_{2}}\]evolved is [MHCET 2004] |
| A. | \[11.2\ d{{m}^{3}}\] |
| B. | \[5.6\,d{{m}^{3}}\] |
| C. | \[22.4\ d{{m}^{3}}\] |
| D. | \[1.0\ d{{m}^{3}}\] |
| Answer» C. \[22.4\ d{{m}^{3}}\] | |
| 6012. |
The amount of silver deposited by passing 241.25 coulomb of current through silver nitrate solution is [MHCET 2003] |
| A. | 2.7 g |
| B. | 2.7 mg |
| C. | 0.27 g |
| D. | 0.54 g |
| Answer» D. 0.54 g | |
| 6013. |
A certain current liberated 0.504 gm of hydrogen in 2 hours. How many grams of copper can be liberated by the same current flowing for the same time in a copper sulphate solution [NCERT 1973, 77; CPMT 1979, 89; AIIMS 1998] |
| A. | 12.7 gm |
| B. | 15.9 gm |
| C. | 31.8 gm |
| D. | 63.5 gm |
| Answer» C. 31.8 gm | |
| 6014. |
Which solution will show highest resistance during the passage of current [BHU 2001] |
| A. | 0.05 N \[NaCl\] |
| B. | 2 N \[NaCl\] |
| C. | 0.1 N \[NaCl\] |
| D. | 1 N \[NaCl\] |
| Answer» C. 0.1 N \[NaCl\] | |
| 6015. |
The quantity of electricity required to liberate \[112\,\,\,c{{m}^{3}}\] of hydrogen at STP from acidified water is [KCET (Med.) 2001] |
| A. | 0.1 Faraday |
| B. | 1 Faraday |
| C. | 965 Coulomb |
| D. | 96500 Coulomb |
| Answer» D. 96500 Coulomb | |
| 6016. |
The unit for the electric current is [KCET (Med.) 2001] |
| A. | Ohm |
| B. | Volt |
| C. | Ampere |
| D. | Coulomb |
| Answer» D. Coulomb | |
| 6017. |
If 0.5 amp current is passed through acidified silver nitrate solution for 10 minutes. The mass of silver deposited on cathode, is (eq. wt. of silver nitrate = 108) [AFMC 2001] |
| A. | 0.235 g |
| B. | 0.336 g |
| C. | 0.536 g |
| D. | 0.636 g |
| Answer» C. 0.536 g | |
| 6018. |
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 | |
| 6019. |
A current of 0.25A is passed through \[CuS{{O}_{4}}\] solution placed in voltameter for 45 minutes. The amount of Cu deposited on cathode is (At weight of \[Cu=63.6\]) [BHU 2001] |
| A. | 0.20 g |
| B. | 0.22 g |
| C. | 0.25 g |
| D. | 0.30 g |
| Answer» C. 0.25 g | |
| 6020. |
In order to separate oxygen from one mole of \[{{H}_{2}}O\] the required quantity of coulomb would be [RPET 1999] |
| A. | \[1.93\times {{10}^{5}}\] |
| B. | \[9.6\times {{10}^{4}}\] |
| C. | 1.8 |
| D. | 3.2 |
| Answer» B. \[9.6\times {{10}^{4}}\] | |
| 6021. |
The unit of electrochemical equivalent is [EAMCET 1980] |
| A. | Gram |
| B. | Gram/ampere |
| C. | Gram/coulomb |
| D. | Coulomb/gram |
| Answer» D. Coulomb/gram | |
| 6022. |
Silver is removed electrically from 200 ml of a 0.1 N solution of \[AgN{{O}_{3}}\] by a current of 0.1 ampere. How long will it take to remove half of the silver from the solution [AMU 1999] |
| A. | 16 sec |
| B. | 96.5 sec |
| C. | 100 sec |
| D. | 10 sec |
| Answer» C. 100 sec | |
| 6023. |
The equivalent weight of a certain trivalent element is 20. Molecular weight of its oxide is [KCET 2003] |
| A. | 152 |
| B. | 56 |
| C. | 168 |
| D. | 68 |
| Answer» D. 68 | |
| 6024. |
The atomic weight of \[Fe\] is 56. The weight of Fe deposited from \[FeC{{l}_{3}}\]solution by passing 0.6 Faraday of electricity is [MH CET 2000] |
| A. | 5.6 g |
| B. | 11.2 g |
| C. | 22.4 g |
| D. | 33.6 g |
| Answer» C. 22.4 g | |
| 6025. |
On electrolysis, 1 mole of aluminium will be deposited from its molten salt by [MH CET 2000] |
| A. | 3 moles of electrons |
| B. | 4 moles of electrons |
| C. | 2 moles of electrons |
| D. | 1 mole of electrons |
| Answer» B. 4 moles of electrons | |
| 6026. |
The mass deposited at an electrode is directly proportional to [CPMT 1974; AFMC 1987; MP PET 2000] |
| A. | Atomic weight |
| B. | Equivalent weight |
| C. | Molecular weight |
| D. | Atomic number |
| Answer» C. Molecular weight | |
| 6027. |
When one of ampere current flows for \[1\,\sec \]through a conductor, this quantity of electricity is known as [MP PMT 1993] |
| A. | Faraday |
| B. | Coulomb |
| C. | E.M.F. |
| D. | Ohm |
| Answer» C. E.M.F. | |
| 6028. |
The number of coulombs required for the deposition of 107.870 g of silver is [MP PET/PMT 1998] |
| A. | 96,500 |
| B. | 48,250 |
| C. | 1,93,000 |
| D. | 10,000 |
| Answer» B. 48,250 | |
| 6029. |
The quantity of electricity needed to liberate 0.5 gram equivalent of an element is [CPMT 1988; MP PMT 1997] |
| A. | 48250 Faradays |
| B. | 48250 Coulombs |
| C. | 193000 Faradays |
| D. | 193000 Coulombs |
| Answer» C. 193000 Faradays | |
| 6030. |
When electricity is passed through the solution of \[AlC{{l}_{3}},\,\,13.5\,\,gm\] of \[Al\] are deposited. The number of Faraday must be [NCERT 1974; MP PET 1992; MP PMT 1994] |
| A. | 0.50 |
| B. | 1.00 |
| C. | 1.50 |
| D. | 2.00 |
| Answer» D. 2.00 | |
| 6031. |
The number of Faradays needed to reduce 4 gram equivalents of \[C{{u}^{++}}\] to \[Cu\] metal will be [BHU 1981] |
| A. | 1 |
| B. | 2 |
| C. | 1/2 |
| D. | 4 |
| Answer» E. | |
| 6032. |
An apparatus used for the measurement of quantity of electricity is known as a [BHU 1979] |
| A. | Calorimeter |
| B. | Cathetometer |
| C. | Coulometer |
| D. | Colorimeter |
| Answer» D. Colorimeter | |
| 6033. |
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. | |
| 6034. |
Three faradays of electricity are passed through molten \[A{{l}_{2}}{{O}_{3}}\], aqueous solution of \[CuS{{O}_{4}}\] and molten \[NaCl\] taken in different electrolytic cells. The amount of \[Al,\,Cu\] and \[Na\] deposited at the cathodes will be in the ratio of [BHU 1990] |
| A. | 1 mole : 2 mole : 3 mole |
| B. | 3 mole : 2 mole : 1mole |
| C. | 1 mole : 1.5 mole : 3 mole |
| D. | 1.5 mole : 2 mole : 3 mole |
| Answer» D. 1.5 mole : 2 mole : 3 mole | |
| 6035. |
The number of electrons required to deposit 1gm atom of aluminium (at. wt. = 27) from a solution of aluminium chloride will be (where N is Avogadro's number) [AIIMS 1992] |
| A. | 1 N |
| B. | 2 N |
| C. | 3 N |
| D. | 4 N |
| Answer» D. 4 N | |
| 6036. |
A certain quantity of electricity is passed through an aqueous solution of \[AgN{{O}_{3}}\] and cupric salt solution connected in series. The amount of \[Ag\] deposited is \[1.08\,gm\], the amount of copper deposited is (atomic weight of Cu = 63.5; Ag = 108) [EAMCET 1986] |
| A. | 0.6454 g |
| B. | 6.354 g |
| C. | 0.3177 g |
| D. | 3.177 g |
| Answer» D. 3.177 g | |
| 6037. |
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 | |
| 6038. |
96500 coulombs of electric current liberates from \[CuS{{O}_{4}}\] solution [MP PMT 1995] |
| A. | \[63.5\,gm\,Cu\] |
| B. | \[31.75\,gm\,Cu\] |
| C. | \[96500\,gm\,Cu\] |
| D. | \[100\,gm\,Cu\] |
| Answer» C. \[96500\,gm\,Cu\] | |
| 6039. |
The required charge for one equivalent weight of silver deposite on cathode is [Roorkee 1995] |
| A. | \[9.65\times {{10}^{7}}C\] |
| B. | \[9.65\times {{10}^{4}}C\] |
| C. | \[9.65\times {{10}^{3}}C\] |
| D. | \[9.65\times {{10}^{5}}C\] |
| Answer» C. \[9.65\times {{10}^{3}}C\] | |
| 6040. |
Faraday has the dimensions of [MP PET 1995] |
| A. | Coulombs |
| B. | Coulomb equivalent |
| C. | Coulomb per equivalent |
| D. | Coulomb per degree Kelvin |
| Answer» D. Coulomb per degree Kelvin | |
| 6041. |
During electrolysis of fused aluminium chloride \[0.9\,gm\] of aluminium was deposited on the cathode. The volume of chlorine liberated at the anode will be |
| A. | 2.24 litres |
| B. | 11.2 litres |
| C. | 1.12 litres |
| D. | 5.6 litres |
| Answer» B. 11.2 litres | |
| 6042. |
The atomic weight of \[Al\] is 27. When a current of 5 Faradays is passed through a solution of \[A{{l}^{+++}}\]ions, the weight of \[Al\] deposited is [NCERT 1984] |
| A. | 27 gm |
| B. | 36 gm |
| C. | 45 gm |
| D. | 39 gm |
| Answer» D. 39 gm | |
| 6043. |
When 96500 coulomb of electricity is passed through a copper sulphate solution, the amount of copper deposited will be [MP PMT 1996] |
| A. | 0.25 mol |
| B. | 0.50 mol |
| C. | 1.00 mol |
| D. | 2.00 mol |
| Answer» C. 1.00 mol | |
| 6044. |
The electrolytic cells, one containing acidified ferrous chloride and another acidified ferric chloride are connected in series. The ratio of iron deposited at cathodes in the two cells when electricity is passed through the cells will be [CPMT 1989] |
| A. | 3 : 1 |
| B. | 2 : 1 |
| C. | 1 : 1 |
| D. | 3 : 2 |
| Answer» E. | |
| 6045. |
The number of electrons passing per second through a cross-section of copper wire carrying \[{{10}^{-6}}\] amperes of current per second is found to be [EAMCET 1985] |
| A. | \[1.6\times {{10}^{-19}}\] |
| B. | \[6\times {{10}^{-35}}\] |
| C. | \[6\times {{10}^{-16}}\] |
| D. | \[6\times {{10}^{12}}\] |
| Answer» E. | |
| 6046. |
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 | |
| 6047. |
Coulomb is equal to [Orissa JEE 2002] |
| A. | ampere ´ second |
| B. | ampere ´ minute |
| C. | watt ´ second |
| D. | volt ´ second |
| Answer» B. ampere ´ minute | |
| 6048. |
The energy required to release 1 electron from \[H{{e}^{+}}\]is??. [Orissa JEE 2002] |
| A. | + 54.4 eV |
| B. | ? 13.6 eV |
| C. | + 27.2 eV |
| D. | Cannot be predicted |
| Answer» C. + 27.2 eV | |
| 6049. |
The number of electrons involved in redox reactions when a Faraday of electricity is passed through an electrolyte in solution is [NCERT 1982; Pb. PMT 2002] |
| A. | \[6\times {{10}^{23}}\] |
| B. | \[6\times {{10}^{-23}}\] |
| C. | 96500 |
| D. | \[8\times {{10}^{19}}\] |
| Answer» B. \[6\times {{10}^{-23}}\] | |
| 6050. |
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 | |