JEE Main Chemistry: Electrochemistry Practice Questions

14 questions with answers and step-by-step solutions. Tap any question to see the full worked solution.

Q1.
$W ha t i s t h e v a l u eo f t h ece l l co n s t an t i f t h eco n d u c t i v i t y i s 0.01 S c m^{-} 1 an d t h er es i s t an ce i s 100 o hm ?$
Easy
Q2.
$What is the unit of molar conductivity?$
Easy
Q3.
$In a Daniel cell, which metal acts as the anode?$
Easy
Q4.
$Which of the following is a strong electrolyte?$
Easy
Q5.
$What is the standard electrode potential of the standard hydrogen electrode?$
Easy
Q6.
$The standard electrode potential for the reduction of Fe3+ to Fe2+ is 0.77 V and for Fe2+ to Fe is -0.44 V. The standard electrode potential for the reduction o$
Medium
Q7.
$How much charge is required to reduce 1 mole of MnO4- to Mn2+?$
Medium
Q8.
$For the reaction 2Fe3+ + 2I- -> 2Fe2+ + I2, the standard EMF is 0.236 V at 298 K. Calculate the equilibrium constant.$
Medium
Q9.
$The molar conductivity of a 0.025 M methanoic acid is 46.1 S cm2 mol-1. Calculate the degree of dissociation if lambda zero for H+ and HCOO- are 349.6 and 54.6$
Medium
Q10.
$Calculate the EMF of the cell Zn | Zn2+ (0.1 M) || Ag+ (0.01 M) | Ag at 298 K. Given E0 Zn2+/Zn = -0.76 V and E0 Ag+/Ag = 0.80 V.$
Medium
Q11.
$For the cell reaction Zn(s) + Cu2+(aq) -> Zn2+(aq) + Cu(s), the standard cell potential is 1.10 V. If the concentration of Zn2+ is 0.1 M and Cu2+ is 0.01 M at 2$
Hard
Q12.
$What is the standard Gibbs free energy change for the cell reaction involving 2 moles of electrons with a standard cell potential of 0.5 V?$
Hard
Q13.
$A current of 0.5 A is passed through a solution of CuSO4 for 20 minutes. What is the mass of copper deposited at the cathode? (Atomic mass of Cu = 63.5 g/mol, F$
Hard
Q14.
$The molar conductivity of a 0.025 M methanoic acid solution is 46.1 S cm2/mol. Calculate the degree of dissociation if the limiting molar conductivities of H+ a$
Hard

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