Retro (Past 13 Year) IIT-JEE Advanced (Electrochemistry) - JEE MCQ

Passage for Q. Nos. (4-5)

The electrochemical cell shown below is a concentration cell. M | M²⁺ (saturated solution of a sparingly soluble salt, MX₂) | | M²⁺ (0.001 mol dm^-3) |M The emf of the cell depends on the difference in concentration of M²⁺ ions at the two electrodes. The emf of the cell at 298K is 0.059 V.

Q.

The solubility product (K_sp ; mol³dm^-9) of MX₂ at 298 K based on the information available the given concentration cell is (take 2.303x R x 298 / F= 0.059 V)

The electrochemical cell shown below is a concentration cell. M | M²⁺ (saturated solution of a sparingly soluble salt, MX₂) | | M²⁺ (0.001 mol dm^-3) |M The emf of the cell depends on the difference in concentration of M²⁺ ions at the two electrodes. The emf of the cell at 298K is 0.059 V.

Q.

The value of ΔG (kJ mol^-1) for the given cell is (take 1 F= 96500 C mol^-1)

Consider the following cell reaction,

At [Fe²⁺] = 10^-3 M, p(O₂) = 0.1 atm and pH = 3, the cell potential at 25°C is

(2011, Only One Option Correct Type)

AgNO₃ (aqueous) was added to an aqueous KCI solution gradually and the conductivity of the solution was measured. The plot of conductance (A) versus the volume of AgNO₃ is

(2011, Only One Option Correct Type)

Passage for Q. N os. (8-9)

The concentration of potassium ions inside a biological cell is at least twenty times higher than the outside. The resulting potential difference across the cell is important in several processes such as transmission of nerve impulses and maintaining the ion balance. A simple model for such a concentration cell involving a metal M is M(s) | M⁺ (aq 0.05 molar) | | M⁺ (ag; 1 molar) | M(s).
For the above electrolytic cell the magnitude of the cell potential | E_cell  | = 70 mV.

Q.

For the above cell

The concentration of potassium ions inside a biological cell is at least twenty times higher than the outside. The resulting potential difference across the cell is important in several processes such as transmission of nerve impulses and maintaining the ion balance. A simple model for such a concentration cell involving a metal M is M(s) | M⁺ (aq 0.05 molar) | | M⁺ (ag; 1 molar) | M(s).
For the above electrolytic cell the magnitude of the cell potential | E_cell  | = 70 mV.

Q.

If the 0.05 molar solution of M⁺ is replaced by a 0.0025 molar M⁺ solution, then the magnitude of the cell potential would be

For the reduction of NO₃^- ion in an aqueous solution E° is + 0.96 V. Values of E° for some metal ions are given below

The pair(s) of metals that is(are) oxidised by NO₃^- in aqueous solution is(are)

(2009, One or More than One Options Correct Type)

Electrolysis of dilute aqueous NaCI solution was carried out by passing 10 mA current. The time required to liberate 0.01 mole of H₂ gas at the cathode is (1 F = 96500 C mol^-1)

(2008,Only One Option Correct Type)

Passage for Q. Nos. (12-13)

Redox reaction play a vital role in chemistry and biology. The values of standard redox potential (E°) of two half-cell reactions decide which way the reaction is expected to proceed. A simple example is a Daniell cell in which zinc goes into solution and copper gets deposited. Given below are a set of half-cell reactions (acidic medium) along with their E° (V with respect to normal hydrogen electrode) values.

Q.

Among the following, identify the correct statement.

Redox reaction play a vital role in chemistry and biology. The values of standard redox potential (E°) of two half-cell reactions decide which way the reaction is expected to proceed. A simple example is a Daniell cell in which zinc goes into solution and copper gets deposited. Given below are a set of half-cell reactions (acidic medium) along with their E° (V with respect to normal hydrogen electrode) values.

Q.

While Fe³⁺ is stable, Mn³⁺ is not stable in acid solution because

Passage for Q. Nos. (14-16)

Tollen’s reagent is used for the detection of aldehydes. When a solution of AgNO₃ is added to glucose with NH₄OH, then gluconic acid is formed.

Q.

Find In K of this reaction

Tollen’s reagent is used for the detection of aldehydes. When a solution of AgNO₃ is added to glucose with NH₄OH, then gluconic acid is formed.

Q.

When ammonia is added to the solution, pH is raised to 11. Which half-cell reaction is affected by pH and by how much?

Tollen’s reagent is used for the detection of aldehydes. When a solution of AgNO₃ is added to glucose with NH₄OH, then gluconic acid is formed.

Q.

Ammonia is always added in this reaction. Which of the following must be incorrect?

We have taken a saturated solution of AgBr, K_sp is 12 x 10^-14 If 10^-7 M of AgNO₃ are added to 1 L of this solution, find conductivity (specific conductance) of this solution in terms of 10^-7 Sm^-1 units.

(2006, Subjective Type)

The half-cell reactions for rusting of iron are: 

ΔG° (in kJ) for the reaction is

(2005, Only One Option Correct Type)