ECAT Chemistry Chapter 10 Electrochemistry With Answers

ECAT Chemistry Chapter 10 Electrochemistry

Sr. # Questions Answers Choice
1 The difference of potential of two electrodes when concentration of solution is 1M each at 25°C and1 atm is called :

 Cell reaction. Electrode potential. Cell voltage. Standard cell potential.
2 Which of the following statement is incorrect about SHE(Standard hydrogen electrode): Reduction potential of Cu<sup>+2</sup> is smaller than H<sup>+</sup>ions whenit is coupled with copper electrode. gas is passed in it at 1 atm pressure. Its oxidation potential and reduction potential is zero. It is made of platinum wire dipped in HCl solution
3 A half reaction can be defines as : It always occurs at cathode. Involves only half of a mole of electrolyte. Occurs at one of the electrode. Goes only half way to completion.
4 Reduction or oxidation potential of standard hydrogen electrode is : 0.0 Volt 0.8Volt 1.0Volt 1.8Volt
5 Cell potential depends upon : Concentration of ions Nature of electrolyte Temperature All of above
6 The best electrode used in salt bridge is KCl. Which other electrolyte an also be used for the purpose : NaCl <p class="MsoNormal">NH<sub>4</sub>NO<sub>3</sub><o:p></o:p></p> <p class="MsoNormal">KNO<sub>3</sub><o:p></o:p></p> <p class="MsoNormal">NaNO<sub>3</sub><o:p></o:p></p>
7 K,Ca and Li metals may be arranged in decreasing order of their reduction potential as : Li, k, Ca Ca, K, Li Li, Ca, K K, Ca, Li
8 When aluminium electrode is coupled with copper electrode in a galvanic cell : Reduction takes place at aluminium electrode. Oxidation takes place at copper electrode. Reduction takes place at copper electrode. Both (a) and (c)
9 When fused PbBr2 is electrolyzed : Lead appears at anode. Lead appears at cathode. Bromine appears at cathode. Lead appears at both electrodes.
10 The cell in which a non-spontaneous redox reaction takes place as a result electricity is known as : Electrolytic cell. Voltaic cell. Daniel cell. Dry cell.
11 A cell in which electric current is produced as a result spontaneous redox reaction is called : Dry cell Electrolytic cell Galvanic cell Standard cell
12 Sodium can be obtained by : Electrolysis of acidified water. By heating NaCl and water at 100<span style="color: rgb(84, 84, 84); font-family: Arial, sans-serif;">°</span><p class="MsoNormal"><sub><o:p></o:p></sub></p> Electrolysis of molten sodium chloride. Electrolysis of aqueous sodium chloride.
13 What are the products electrolysis of aqueous sodium chloride at two electrodes Chlorine at anode and oxygen at cathode. Hydrogen at anode and chlorine at cathode. Chlorine at anode and hydrogen at cathode. Chlorine at anode and sodium at cathode.
14 Which of the following correctly describes the process occurring at the electrodes when molten NaCl is electrolyzed: No reaction at anode, reduction at cathode. No reaction at cathode, oxidation at anode. Oxidation at anodes, reduction at cathode. Oxidation at cathode, reduction at anode.
15 Which of the following yield both hydrogen and chlorine on electrolysis: Electrolysis of acidified water. Electrolysis of molten NaCl Electrolysis of aqueous NaCl Electrolysis of saline water
16 The function of salt bridge is : To increase movement onions. To increase the emf of cell. To decrease the temperate To maintain electrical neutrality
17 During electrolysis, electrons are : Lost by anions and gained by cations Gained by anions and lost by cations Gained only Lost only
18 During electrolysis, the reaction that takes place at cathode is : Reduction Both (a) and (c) Oxidation No reaction occurs
19 Which of the following cannot conduct electricity : NaCl fused. NaCl<span style="font-family: Arial, sans-serif; font-size: 10.5pt; vertical-align: sub;">(aq)</span><p class="MsoNormal"><sub><o:p></o:p></sub></p> <span style="font-family: Arial, sans-serif; font-size: 10.5pt; vertical-align: sub;"></span>NaCl<span style="font-family: Arial, sans-serif; font-size: 10.5pt; vertical-align: sub;">(Solid)</span><p class="MsoNormal"><sub><o:p></o:p></sub></p><p class="MsoNormal"><o:p></o:p></p> Both (b) and (c)
20 In electrolytic cells, the chemical changes may be : Either spontaneous or non-spontaneous Always spontaneous Always non-spontaneous More spontaneous and less non-spontaneous.
21 When aqueous NaCl is electrolyzed, which of the following ions get discharged at anode : <p class="MsoNormal"><span style="font-size: 10.5pt; line-height: 107%; font-family: Arial, sans-serif; background-image: initial; background-position: initial; background-size: initial; background-repeat: initial; background-attachment: initial; background-origin: initial; background-clip: initial;">H<sup>+</sup><o:p></o:p></span></p> <p class="MsoNormal"><span style="font-size: 10.5pt; line-height: 107%; font-family: Arial, sans-serif; background-image: initial; background-position: initial; background-size: initial; background-repeat: initial; background-attachment: initial; background-origin: initial; background-clip: initial;">Na<sup>+</sup><o:p></o:p></span></p> <p class="MsoNormal"><span style="font-size: 10.5pt; line-height: 107%; font-family: Arial, sans-serif; background-image: initial; background-position: initial; background-size: initial; background-repeat: initial; background-attachment: initial; background-origin: initial; background-clip: initial;">OH<sup>-</sup><o:p></o:p></span></p> <p class="MsoNormal"><span style="font-size: 10.5pt; line-height: 107%; font-family: Arial, sans-serif; background-image: initial; background-position: initial; background-size: initial; background-repeat: initial; background-attachment: initial; background-origin: initial; background-clip: initial;">Cl<sup>-</sup></span><o:p></o:p></p>
22 In an electrolytic cell, the electrons flow from : Cathode to anode or opposite Cathode to anode Anode to cathode Random flow
23 Electrolysis is used for : Manufacture of caustic soda Refining of copper Electroplating All of above
24 Ionization is the process in which ionic compounds when fused or dissolved in water split up into charged particles called : Atoms. Electrons. Protons . Ions
25 Electrolytes in the form of solution or in the fused state have the ability to conduct : Light. Electricity. Ions. Electrons.
26 Metallic conduction is also called as : Ionic conduction. Protonic conduction. Electronic conduction Super conduction
27 Most metals are conductors of electricity because of the : Light weight. Immobility of the electrons. Lustrous surfaces Relatively free movement of their electrons
28 The conversion of chemical energy into electrical energy requires : Electrolytic cell Galvanic cell Voltaic cell Both (b) and (c)
29 Electrochemistry is concerned with the conversion of electrical energy into chemical energy in : Galvanic cell Electrolytic cell Voltaic cell Both (a) and (c)
30 In a hydrogen-oxygen fuel cell, combustion of hydrogen occurs to Generate heat Remove adsorbed oxygen from electrode surfaces Produce High purity water Create potential difference between two electrodes
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