Balbharati solutions for Chemistry 12th Standard HSC for Maharashtra State Board chapter 5 - Electrochemistry [Latest edition]

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Balbharati solutions for Chemistry 12th Standard HSC for Maharashtra State Board chapter 5 - Electrochemistry - Shaalaa.com
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Solutions for Chapter 5: Electrochemistry

Below listed, you can find solutions for Chapter 5 of Maharashtra State Board Balbharati for Chemistry 12th Standard HSC for Maharashtra State Board.


Exercises
Exercises [Pages 117 - 119]

Balbharati solutions for Chemistry 12th Standard HSC for Maharashtra State Board Chapter 5 Electrochemistry Exercises [Pages 117 - 119]

Exercises | Q 1.01 | Page 117

Choose the most correct option.

Two solutions have the ratio of their concentrations 0.4 and ratio of their conductivities 0.216. The ratio of their molar conductivities will be ______.

  • 0.54

  • 11.574

  • 0.0864

  • 1.852

Exercises | Q 1.02 | Page 117

Choose the most correct option.

On diluting the solution of an electrolyte _______.

  • both λ and k increase

  • both λ and k decrease

  • λ increases and k decreases

  • λ decreases and k increases

Exercises | Q 1.03 | Page 117

Choose the most correct option.

1 S m2 mol-1 is equal to _______.

  • 10–4 S m2 mol–1

  • 104 Ω –1 cm2 mol–1

  • 10–2 S cm2 mol–1

  • 102 Ω –1 cm2 mol–1

Exercises | Q 1.04 | Page 117

Choose the most correct option.

The standard potential of the cell in which the following reaction occurs:
H2 (g,1 atm) + Cu2+ (1M) → 2H+ (1M) + Cu(s),
`("E"_"Cu"^circ = 0.34 "V")` is

  • - 0.34 V

  • 0.34 V

  • 0.17 V

  • - 0.17 V

Exercises | Q 1.05 | Page 117

Choose the most correct option.

For the cell,

Pb(s) |Pb2+ (1 M)| |Ag+ (1 M)| Ag(s),

if concentration of an ion in the anode compartment is increased by a factor of 10, the emf of the cell will

  • increase by 10 V

  • increase by 0.0296 V

  • decrease by 10 V

  • decrease by 0.0296 V

Exercises | Q 1.06 | Page 117

Choose the most correct option.

Consider the half reactions with standard potentials _______.

i. \[\ce{Ag^{+}_{ (aq)} + e^- -> Ag_{(s)}E°}\]= 0.8 V

ii. \[\ce{I_{2(s)} + 2e^- -> 2I^{-}_{ (aq)} E°}\] = 0.53 V

iii. \[\ce{Pb^{2+}_{ (aq)} + 2e^- -> pb_{(s)} E°}\]= - 0.13 V

iv. \[\ce{Fe^{2+} + 2e^- -> Fe_{(s)} E°}\]= - 0.44 V

The strongest oxidising and reducing agents respectively are

  • Ag and Fe2+

  • Ag+ and Fe 

  • Pb2+ and I

  • I2 and Fe2+ 

Exercises | Q 1.07 | Page 117

Choose the most correct option.

For the reaction:

Ni(s) + Cu2+ (1 M) → Ni2+ (1 M) + Cu(s),

`"E"_"cell"^circ` = 0.57 V, Δ G° of the reaction is

  • 110 kJ

  • - 110 kJ

  • 55 kJ

  • - 55 kJ

Exercises | Q 1.08 | Page 117

Choose the most correct option.

Which of the following is not correct?

  • Gibbs energy is an extensive property

  • Electrode potential or cell potential is an intensive property

  • Electrical work = – ΔG

  • If half-reaction is multiplied by a numerical factor, the corresponding E° value is also multiplied by the same factor.

Exercises | Q 1.09 | Page 117

Choose the most correct option.

The oxidation reaction that takes place in lead storage battery during discharge is

  • `"Pb"_(("aq"))^(2+) + "SO"_(4("aq"))^(2-) -> "PbSO"_(4("s"))`

  • `"PbSO"_(4("s")) + 2"H"_2"O"_(("l")) -> "PbO"_(2("s")) + 4"H"_(("aq"))^+ + "SO"_(4("aq"))^(2-) + 2"e"^-`

  • `"Pb"_("s") + "SO"_(4("aq"))^(2-) -> "PbSO"_(4("s")) + 2"e"^-`

  • `"PbSO"_(4("s")) + 2"e"^-  -> "Pb"_("s") + "SO"_(4("aq"))^(2-)`

Exercises | Q 1.1 | Page 118

Choose the most correct option.

Which of the following expressions represent molar conductivity of Al2(SO4)3?

  • `3 lambda_("Al"^(3+))^0 + 2lambda _("SO"_4^(2-))^0`

  • `2 lambda_("Al"^(3+))^0 + 3 lambda _("SO"_4^(2-))^0`

  • `1//3 lambda_("Al"^(3+))^0 + 1//2lambda _("SO"_4^(2-))^0`

  • `lambda_("Al"^(3+))^0 + lambda _("SO"_4^(2-))^0`

Exercises | Q 2.01 | Page 118

What is a cell constant? What are its units? How is it determined experimentally?

Exercises | Q 2.02 | Page 118

Answer the following in one or two sentences.

Write the relationship between conductivity and molar conductivity and hence unit of molar conductivity.

Exercises | Q 2.03 | Page 118

Answer the following in one or two sentences.

Write the electrode reactions during electrolysis of molten KCl.

Exercises | Q 2.04 | Page 118

Answer the following in one or two sentences.

Write any two functions of salt bridge.

Exercises | Q 2.05 | Page 118

Answer the following in one or two sentences.

What is the standard cell potential for the reaction?

\[\ce{2Al(s) + 3Ni^{2⊕}(1M) -> 2Al^{3⊕}(1 M) + 3Ni(s)}\]

if `"E"_"Ni"^0` = −0.25 V and `"E"_"Al"^0` = −1.66 V

Exercises | Q 2.06 | Page 118

Answer the following in one or two sentences.

Write Nernst equation. What part of it represents the correction factor for nonstandard state conditions?

Exercises | Q 2.07 | Page 118

Answer the following in one or two sentences.

Under what conditions the cell potential is called standard cell potential?

Exercises | Q 2.08 | Page 118

Answer the following in one or two sentences.

Formulate a cell from the following electrode reactions:

`"Au"_(("aq"))^(3+) + 3"e"^(-) -> "Au"_(("s"))`

Mg(s) → `"Mg"_(("aq"))^(2+)` + 2e-

Exercises | Q 2.09 | Page 118

Answer the following in one or two sentences.

How many electrons would have a total charge of 1 coulomb?

Exercises | Q 2.1 | Page 118

Answer the following in one or two sentences.

What is the significance of the single vertical line and double vertical line in the formulation galvanic cell?

Exercises | Q 3.01 | Page 118

Answer the following in brief.

Explain the effect of dilution of the solution on conductivity.

Exercises | Q 3.02 | Page 118

Answer the following in brief.

What is a salt bridge?

Exercises | Q 3.03 | Page 118

Answer the following in brief.

Write electrode reactions for the electrolysis of aqueous NaCl.

Exercises | Q 3.04 | Page 118

Answer the following in brief.

How many moles of electrons are passed when 0.8-ampere current is passed for 1 hour through molten CaCl2?

Exercises | Q 3.05 | Page 118

Answer the following in brief.

Construct a galvanic cell from the electrodes Co3+ | Co and Mn2+/Mn. `"E"_"Co"^circ` = 1.82 V, `"E"_"Mn"^circ` = –1.18 V. Calculate `"E"_"cell"^circ`

Exercises | Q 3.06 | Page 118

Answer the following in brief.

Using the relationship ΔG° of cell reaction and the standard potential associated with it, how will you show that the electrical potential is an intensive property?

Exercises | Q 3.07 | Page 118

Derive the relationship between standard cell potential and equilibrium constant of cell reaction.

Exercises | Q 3.08 | Page 118

Answer the following in brief.

It is impossible to measure the potential of a single electrode. Comment.

Exercises | Q 3.09 | Page 118

Answer the following in brief.

Why do the cell potential of lead accumulators decrease when it generates electricity? How the cell potential can be increased?

Exercises | Q 3.1 | Page 118

Answer the following in brief.

Write the electrode reactions and net cell reaction in NICAD battery.

Exercises | Q 4.01 | Page 118

Answer the following:

What is Kohlrausch law of independent migration of ions? How is it useful in obtaining molar conductivity at zero concentration of a weak electrolyte? Explain with an example.

Exercises | Q 4.02 | Page 118

Answer the following:

Explain electrolysis of molten NaCl.

Exercises | Q 4.03 | Page 118

Answer the following:

What current strength in amperes will be required to produce 2.4 g of Cu from CuSO4 solution in 1 hour? Molar mass of Cu = 63.5 g mol–1.

Exercises | Q 4.04 | Page 118

Answer the following:

Equilibrium constant of the reaction,

`2"Cu"_(("aq"))^+ -> "Cu"_(("aq"))^(2+) + "Cu"_(("s"))` is 1.2 × 106.

What is the standard potential of the cell in which the reaction takes place?

Exercises | Q 4.05 | Page 119

Answer the following:

Calculate emf of the cell:

Zn(s) |Zn2+ (0.2 M)||H+ (1.6 M)| H2(g, 1.8 atm)| Pt at 25 °C.

Exercises | Q 4.06 | Page 119

Answer the following:

Calculate emf of the cell at 25 °C.

Zn(s) |Zn2+ (0.08 M)| |Cr3+ (0.1 M)| Cr

`"E"_"Zn"^circ` = - 0.76 V, `"E"_"Cr"^circ` = - 0.74 V

Exercises | Q 4.07 | Page 119

What is a cell constant? What are its units? How is it determined experimentally?

Exercises | Q 4.08 | Page 119

Answer the following:

How will you calculate the moles of electrons passed and mass of the substance produced during electrolysis of a salt solution using reaction stoichiometry?

Exercises | Q 4.09 | Page 119

Answer the following:

Write the electrode reactions when lead storage cell generates electricity. What are the anode and cathode and write the electrode reactions during its recharging?

Exercises | Q 4.1 | Page 119

Answer the following:

What are anode and cathode of H2 - O2 fuel cell? Name the electrolyte used in it. Write electrode reactions and net cell reaction taking place in the fuel cell.

Exercises | Q 4.11 | Page 119

Answer the following:

What are anode and cathode for Leclanche' dry cell?

Exercises | Q 4.12 | Page 119

Answer the following:

Identify oxidising agents and arrange them in order of increasing strength under standard state conditions. The standard potentials are given in parenthesis.

Al  (–1.66V), Al3+(–1.66V),  Cl2  (1.36V),  Cd2+ (–0.4V), Fe (–0.44V),  I2 (0.54V),  Br- (1.09V).

Exercises | Q 4.13 | Page 119

Answer the following:

Which of the following species are reducing agents? Arrange them in order of increasing strength under standard state conditions. The standard potentials are given in parenthesis.

K (–2.93V),  Br2(1.09V), Mg(–2.36V), Ce3+(1.61V), Ti2+(–0.37V), Ag+ (0.8 V), Ni (–0.23V).

Exercises | Q 4.14 | Page 119

Answer the following:

Predict whether the following reaction would occur spontaneously under standard state condition.

`"Ca"_(("s")) + "Cd"_(("aq"))^(2+) -> "Ca"_(("aq"))^(2+) + "Cd"_(("s"))`

Exercises | Q 4.14 | Page 119

Answer the following:

Predict whether the following reaction would occur spontaneously under standard state condition.

`2"Br"_(("aq"))^(-) + "Sn"_(("aq"))^(2+) -> "Br"_(2("l")) + "Sn"_(("s"))`

Exercises | Q 4.14 | Page 119

Answer the following:

Predict whether the following reaction would occur spontaneously under standard state condition.

\[\ce{2Ag_{(s)} + Ni^{2+}_{ (aq)} -> 2Ag^{+}_{ (aq)} + Ni_{(s)}}\]

Solutions for Chapter 5: Electrochemistry

Exercises
Balbharati solutions for Chemistry 12th Standard HSC for Maharashtra State Board chapter 5 - Electrochemistry - Shaalaa.com

Balbharati solutions for Chemistry 12th Standard HSC for Maharashtra State Board chapter 5 - Electrochemistry

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Concepts covered in Chemistry 12th Standard HSC for Maharashtra State Board chapter 5 Electrochemistry are Electrochemistry, Electric Conduction, Electrical Conductance of Solution, Electrochemical Cells, Electrolytic Cell, Galvanic or Voltaic Cell, Electrode Potential and Cell Potential, Thermodynamics of Galvanic Cells, Reference Electrodes, Galvanic Cells Useful in Day-to-day Life, Fuel Cells, Electrochemical Series (Electromotive Series).

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Get the free view of Chapter 5, Electrochemistry Chemistry 12th Standard HSC for Maharashtra State Board additional questions for Mathematics Chemistry 12th Standard HSC for Maharashtra State Board Maharashtra State Board, and you can use Shaalaa.com to keep it handy for your exam preparation.

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