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Redox Reactions And Electrochemistry Mock Tests

30 questions available

Redox Reactions And Electrochemistry Mock Test 1

Questions: 30

Sample Questions

JEE Main Chemistry
Delta G for Cu2+ + 2e- -> Cu is: (E = +0.34 V, F = 96500 C/mol)
A -65.8 kJ
B +65.8 kJ
C -32.9 kJ
D +32.9 kJ
JEE Main Chemistry
Which of the following is a secondary battery?
A Lead storage battery
B H2-O2 fuel cell
C Daniell cell
D Dry cell
JEE Main Chemistry
The standard electrode potential (E°) for the cell: Zn(s) | Zn²⁺(1 M) || Cu²⁺(1 M) | Cu(s) is +1.10 V. If the concentration of Zn²⁺ is increased to 10 M while Cu²⁺ remains at 1 M, the cell potential at 298 K will be approximately:
A 1.07 V
B 1.13 V
C 1.10 V
D 1.01 V
JEE Main Chemistry
The process of electrolytic refining of copper uses:
A Impure Cu as anode, pure Cu as cathode
B Pure Cu as anode, impure Cu as cathode
C CuSO4 as anode, H2SO4 as cathode
D Copper as both electrodes
JEE Main Chemistry
The number of moles of electrons transferred when 1 mole of Al₂O₃ is formed from Al and O₂ is:
A 2
B 3
C 4
D 6
JEE Main Chemistry
The number of moles of electrons required to reduce 1 mole of MnO₄⁻ to Mn²⁺ in acidic medium is:
A 3
B 5
C 7
D 2
JEE Main Chemistry
The standard electrode potential of a cell Zn|Zn²⁺(1 M)||Cu²⁺(1 M)|Cu is 1.10 V. If E°(Cu²⁺/Cu) = +0.34 V, the standard electrode potential of Zn²⁺/Zn is:
A -0.76 V
B -1.44 V
C +0.76 V
D +1.44 V
JEE Main Chemistry
The emf of the cell Zn(s) | Zn²⁺(0.01 M) || Cu²⁺(1.0 M) | Cu(s) at 298 K is: (E°cell = 1.10 V, 2.303RT/F = 0.0591 V)
A 1.13 V
B 1.07 V
C 1.10 V
D 1.16 V

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