MDCAT Chemistry Electrochemistry Test Online

1. What is the molality of a solution prepared by dissolving 5 g of toluene in 250 g of Benzene.

2. The process of electrical coating of one metal on another to protect, decorate or to have a greater resistance to corrosion is called

3. Half cells are interconnected through

4. The equivalent conductivity of 0.1 M week acid is 100 times less than that at infinite dilution. The degree of dissociation is

5. Camphor is often used in molecular mass determination because

6. Molarity of water is

7. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

8. The temperature at which the vapour pressure of a liquid becomes equal to external pressure is

9. Which of the statements given below concerning properties of solution, describe a colligaive effect?

10. Reaction takes place at anode is

11. A smuggler could not carry gold by chemically depositing iron on the gold surface since

12. The + 1 oxidation state of P is found in

13. Equal volumes of ethylene glycol (molar mass = 62) and water (molar mass = 18) are mixed. The depression in freezing point of water is (given Kf of water 1.86 K mol¯¹ kg and specific gravity of ethylene glycol is 1.11)

14. Secondary cell is

15. What will be the density of H₂SO₄ when lead accumulator is recharged?

16. A certain current liberate 0.5 g of hydrogen in 2 h. How many grams of copper can be liberated by the same current flowing for the same time in a copper sulphate solution?

17. The pressure at which water boils at 101.5 °c is

18. Salt bridge transfers

19. The vapour pressure of two liquids ‘P’ and ‘Q’ are 80 and 60 torr respectively. The total vapour pressure of solution obtained by mixing 3 mole of P and 2 mol of Q would be

20. The amount of electricity that can deposit 108 g of silver from silver nitrate solution is

21. In alkaline battery the anode is made up of

22. If liquids A and B form an ideal solution

23. Time required to deposit one millimole of aluminum metal by the passage of 9.65 amperes through molten electrolyte containing aluminum ion is

24. Choose the cell among the following list in which conversation of electrical energy into chemical energy takes place

25. A cell in which chemical energy is converted into electrical energy is called

26. Separation of azeotropic mixture into pure components is carried out by

27. By means of fuel cells, chemical energy may be converted into

28. Electrode potential of Zn is

29. Colligative properties are the properties of

30. Which of the following statements is FALSE?

31. In an electrolytic cell current flows

32. What are the ions present in water?

33. In a solution of CuSO₄ how much time will be required to precipitate 2g copper by 0.5 ampere current?

34. The half-reaction that occurs at the anode during the electrolysis of molten sodium bromide is:

35. Which one of the following is a colligative property?

36. Standard hydrogen electrode has an arbitrarily fixed potential

37. Maximum freezing point falls in

38. Which has maximum oxidation number

39. If 18 g of glucose (C₆H₁₂C₆) is present in 1000 g of an aqueous solution of glucose it is said to be

40. Electricity in voltaic cell is produced due to

41. In a Galvanic cell

42. Which of the substances Na, Hg, S Pt and graphite can be used as electrodes in electrolytic cells having aqueous solution?

43. In alkaline battery anode is made up of

44. Reduction always occurs

45. Density of H₂SO₄ in lead accumulator is

46. Azeotropic mixture of HCl and water has

47. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

48. Molton NaCl conducts electricity due to the presence of

49. Potential of Zn is called

50. 1.0 g of pure calcium carbonate was found to require 50 ml of dilute HCl for complete reaction. The strength of HCl solution is given by

51. The solubility of a gas in water depends upon

52. Density of H₂SO₄ in lead accumulator is

53. A solution contains A, B and C components. The mole fraction A and C are 0.25 and 0.35 respectively. The mole fraction B will be

54. Which of the following (IM) conducts more electricity?

55. Corrosion reactions are

56. The substance having highest conductivity at room temperature among the following is

57. In a chemical reaction, oxidation process involves

58. Corrosion is basically a

59. The standard e.m.f. of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at 25°C. The equilibrium constant of the reaction would be

60. How many g of dibasic acid (mol. wt. 200) should be present in 100 ml of the aqueous solution to give 0.1 Normality?

61. If 5.85 g of NaCl are dissolved in 90g of water, the mole fraction of NaCl is

62. The reference electrode is made by using

63. If the ionic product of a solution is less than the solubility product, the solution is

64. A 0.001 molal solution of [Pt(NH₃)₄Cl₄] in water had a freezing point depression of 0.0054°C. If Kf for water is 1.80, the correct formulation for the above molecule is

65. Anode electrode element always have _________ position in electrochemical series

66. If the salt bridge is not used between two half cells, then the voltage

67. 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

68. When Cu, Ag, Au and Pt are reacted with acids, these metals do not liberate hydrogen, this is due to the reason that

69. The depression of freezing point is directly proportional to

70. A redox reaction involves

71. Oxidation in a chemical reaction involves

72. What is the molarity of H₂SO₄ solution that has density of 1.84 gm/cm³ which was at 35°C and contains 98% by weight?

73. A solution contains 1.2046 x 10²⁴ hydrochloric acid molecules in one dm³ of the solution. The strength of the solution is

74. Which of the following solution of H₂SO₄ is more concentrated?

75. Which of the following is a strong electrolyte?

76. The molality of 2% NaCl. W/W solution is approximately

77. 96500 C of electricity liberates from CuSO₄ solution

78. Solution with same osmotic pressures are called

79. In electrolysis of NaCl when Pt electrode is taken then H₂ is liberated at cathode while with Hg cathode it forms sodium amalgam

80. Equal volumes of 0.1 M AgNO₃ and 0.2 M NaCl are mixed. The concentration of NO¯₃ ions in the mixture will be

81. The degree of dissociation of weak electrolyte increases as

82. Of the following, the metal that cannot be obtained by electrolysis of aqueous solution of their salts are:

83. Decrease in oxidation number is called

84. An oxidizing agent in a chemical reaction in the substance which

85. The conductivity of strong electrolyte

86. An electrolyte

87. The volume of 0.1 M H₂SO₄ required to neutralize completely 40 ml of 0.2 M NaOH solution is

88. Which of the following is the use of electrolysis?

89. Units of molarity are

90. Calculate the percentage by weight if NaCl, if 2.0 g of NaCl is dissolved in 20g of water

91. The osmotic pressure of a dilute solution is directly proportional to the

92. After adding a solute freezing point of solvent decreases to -0.186. Calculate ∆ Tb if Kf = 1.86 and Kb = 0.521

93. The best reducing agent is

94. When electricity is passed through molten Al₂O₃ + Na₃AIF₆ and 13.5 gms of Al are deposited, the number of faraday must be

95. Sea water has 5.65 x 10¯³ g of dissolved oxygen calculate the conclusion of oxygen in sea water in ppx

96. The number of coulombs required for the deposition of 107.870 g of silver is

97. Pure water does not conduct electricity because it

98. Oxidation state of hydrogen in CaH₂ is

99. When a metal is dipped in 1 molar of its solution at 298k, then potential set up is called

100. Which of the following is the strongest oxidizing agent?

101. A dry alkaline cell has porous Zn anode & MnO₂ as cathode the electrolyte used is

102. 2.5 faradays of electricity is passed through solution of CuSO₄. The number of gram equivalents of copper deposited on the cathode would be

103. Prevention of corrosion of iron by Zn coating is called

104. For spontaneity of a cell, which is correct?

105. The electrode with more negative value of reduction potential acts as

106. H₂ gas in SHE is filled at a pressure of

107. Best way to prevent rusting iron is by

108. At room temperature, the mole fraction of a solution in 0.25 and the vapour pressure of the solvent is 0.80 atm. Then the lowering of vapour pressure is

109. Which one of the following will be good conductor of electricity?

110. The strength of solution an element whose electrode potential is to be measured

111. Partial pressure of a solution component is directly proportional to its mole fraction. This statement is known as

112. The relative lowering of vapour pressure is equal to mole fraction of the solute. This law is called:

113. Hydrogen gas is not liberated when the following metal is added to dil. HCI.

114. The osmotic pressure of 1 m solution at 27°C is

115. Electrochemical series is a list of elements arranged into increasing order to either

116. The cathodic reaction in the electrolysis of dil. H₂SO₄ with Pt electrodes is

117. When during electrolysis of a solution of AgNO₃, 9650 coulombs of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be

118. The weight of pure NaOH required to prepare 250 cm³ of 0.1 N solution is

119. In the conversion of Br2 to BrO₃¯¹ the oxidation state of bromine changes from

120. A solution of sodium sulphate was electrolyzed using some inert electrodes. The products at the electrodes are

121. Under the process of rusting of iron, 4Fe + 3O₂ → 2Fe₂O₃, iron is

122. The unit of specific conductivity is

123. Specific conductivity of a solution

124. When molten sodium undergoes electrolysis, the ion reduces is

125. It azeotropic mixture showing positive deviation from Rault’s law, the volume of the mixture is

126. If a salt bridge is removed between the two half cells, the voltage

127. Conductivity (Unit : siemen’s S) is directly proportionally to the area of the vessel and the concentration of the solution in it and is inversely proportional to the length of vessel, then the unit of constant of proportionality is

128. Which substances are mixed to form a buffer solution?

129. When the solute is present in trace quantities the following expression is used?

130. Cathodic reaction in the electrolysis of dil. H₂SO₄ is always

131. The limiting molar conductivities ʌ’ for NaCl, KBr and KCl are 126, 152 and 150 S cm² respectively. The ʌ’ for NaBr is

132. Which of these is not an application of electrolysis?

133. When common salt is dissolved in water

134. In a hydrogen-oxygen fuel cell, combustion of hydrogen occurs to

135. In electrolytic cell, electricity in carried out by

136. The reference calomel electrode is made from which of the following?

137. Which of the following statement is correct for electrolytic cell?

138. Li occupies higher position in the electrochemical series of metals as compared to Cu since

139. The number of moles of a solute in 500 cm³, 3M solution is

140. A current of 9.65 ampere flowing for 10 minutes deposits 3.0 g of the metal which is monovalent. The atomic mass of the metal is

141. The ionic strength of a solution containing 0.1 mole/kg of KCl and 0.2 mole/kg of CuSO₄ is

142. What will be the weight of deposited silver on passing 965 coulombs of electricity in solution of AgNO₃?

143. Chemical used in salt bridge is

144. Out of Cu, Ag, Fe and Zn the metal which can displace all others from their salt solutions is

145. In galvanic cell Zn acts as an anode so its value of standard reduction potential in comparison to coupled electrode would be

146. The cryoscopic constant of water is 1.86. The elevation of B.P for a 0.1m solution of a solute in water is

147. Calculate the amount of charge flowing in 2 minute in a wire of resistance 10 Ω when a potential difference of 20 V is applied

148. The art of electroplating was given by

149. Mole fraction of pure water is

150. The Vant Hoff factor (i) accounts for

151. An aqueous solution of ethanol in water has vapour pressure

152. Stronger the oxidizing agent, greater is the

153. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

154. Which of the following will have the highest boiling point at 1 atm pressure?

155. Choose the best reducing agent among the following

156. Which of the following element act as inert electrode?

157. Metals usually conduct electricity because

158. A cell constant is generally found by measuring the conductivity of aqueous solution of

159. Voltaic cell can be recharged by

160. When electricity is passed through molten electrolyte consisting of alumina and cryolite, 13.5 g of Al are deposited. The number of faradays of electricity passed must be

161. Oxidation number of carbon in NaHCO₃ is

162. The specific conductance of a 0.1 N KCl solution at 23°C is 0.012 ohm¯¹ cm¯¹. The resistance of cell containing the solution at the same temperature was found to be 55 ohm. The cell constant will be

163. In the electrolysis of molten sodium chloride, what is the yellow green gas formed?

164. Electrolysis is the process in which a chemical reaction takes place at the expense of

165. Salt bridge transfers

166. Same amount of electric current is passed through solution if AgNO₃ and HCl. If 1.08 g of silver is obtained in the first case, the amount of hydrogen liberated as S.T.P. in the second case is:

167. A device which converts electrical energy into chemical energy is called

168. Strong reducing agents have

169. Wen quantity of electricity passed is one faraday then the mass deposited at the electrode is equal to

170. An aqueous solution freezes at -0.186°C. (Kf = 1.86, Kb = 0.512). What is the elevation in boiling point?

171. Cathode provides electrons to

172. Which oxide has +2 oxidation number of oxygen?

173. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

174. A 20% solution of NaCl by weight means that

175. Vant Hoff’s factor of Ca(NO₃)₂ is

176. Which one of the following substance when dissolved in water give acidic solution

177. The specific conductance of 0.1 M NaCl solution is 1.06 x 10¯² ohm¯¹mol¯¹. Its molar conductance in ohm¯¹ cm² mol¯¹ is

178. An electric current is passed through silver voltmeter connected to a water voltmeter. The cathode of the silver voltammeter is 0.108 g more at the end of the electrolysis. The volume of oxygen evolved at STP is

179. 50 mL of 10 N H₂SO₄. 25 mL of 12 N HCl and 40 mL of 5N HNO₃ are mixed and the volume of the mixture is made 1000 mL by adding water. The normality of resulting solution will be

180. In a Galvanic cell, the electrons flow from

181. If α is the degree of dissociation of Na₂SO₄ the Vant Hoff’s factor (i) used for calculating the molecular mass is

182. Pick out the wrong statement. In electrochemical cell

183. Standard reduction electrode potential of three metals A, B and C are respectively + 0.05 V, - 3.0 and -1.2V. The reducing power of

184. The molarity of the solution containing x grams (NH₄)SO₄ in 500 cm³ of the solution is 0.6. What is x

185. If 5.85 g of NaCl are dissolved in 90 g of water, the mole fraction of NaCl is

186. The EMF of the cell rection Fe²⁺ + zn = Zn²⁺ + feis

187. Temperature for standard electrode potential is

188. The standard EMF of Daniel cell is 1.10 volt. The maximum electrical work obtained from the Daniel cell is

189. If the standard electrode potential of CU²⁺/Cu electrode is 0.34 V, what is the electrode potential of 0.01 M concentration of Cu²⁺? (T = 298 K)

190. How much of NaOH is required to neutralize 1500 cm³ of 0.1 N HCl?

191. During a redox reaction, an oxidizing agent

192. Alkaline battery has a voltage of