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Chapters
2: Solutions
3: Ionic Equilibria
4: Chemical Thermodynamics
▶ 5: Electrochemistry
6: Chemical Kinetics
7: Elements of Groups 16, 17 and 18
8: Transition and Inner transition Elements
9: Coordination Compounds
10: Halogen Derivatives
11: Alcohols, Phenols and Ethers
12: Aldehydes, Ketones and Carboxylic acids
13: Amines
14: Biomolecules
15: Introduction to Polymer Chemistry
16: Green Chemistry and Nanochemistry
![Balbharati solutions for Chemistry [English] 12 Standard HSC chapter 5 - Electrochemistry - Shaalaa.com](/images/chemistry-english-12-standard-hsc_6:74400b801d4c44ef8e058ff9d9dfe964.jpg "Balbharati solutions for Chemistry [English] 12 Standard HSC chapter 5 - Electrochemistry")
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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 [English] 12 Standard HSC.
Balbharati solutions for Chemistry [English] 12 Standard HSC 5 Electrochemistry Exercises [Pages 117 - 119]
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
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
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
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
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
Consider the half reactions with standard potentials.
- \[\ce{Ag^{\oplus}_{ (aq)} + e^{\ominus} -> Ag_{(s)}E^\circ = 0.8 V}\]
- \[\ce{I2_{(s)} + 2e^\ominus -> 2I^{\ominus}_{(aq)} E^\circ = 0.53V}\]
- \[\ce{Pb^{2\oplus}_{(aq)} + 2e^{\ominus} -> Pb_{(s)} E^\circ = -0.13 V}\]
- \[\ce{Fe^{2\oplus} + 2e^{\ominus} -> Fe_{(s)} E^\circ = -0.44 V}\]
The strongest oxidising and reducing agents respectively are ______.
\[\ce{Ag and Fe^{2\oplus}}\]
\[\ce{Ag^{\oplus} and Fe}\]
\[\ce{Pb^{2\oplus} and I}\]
\[\ce{I2 and Fe^{2\oplus}}\]
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
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.
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-)`
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`
What is a cell constant? What are its units? How is it determined experimentally?
Answer the following in one or two sentences.
Write the relationship between conductivity and molar conductivity and hence unit of molar conductivity.
Answer the following in one or two sentences.
Write the electrode reactions during electrolysis of molten KCl.
Answer the following in one or two sentences.
Write any two functions of salt bridge.
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
Answer the following in one or two sentences.
Write Nernst equation. What part of it represents the correction factor for nonstandard state conditions?
Answer the following in one or two sentences.
Under what conditions the cell potential is called standard cell potential?
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-
Answer the following in one or two sentences.
How many electrons would have a total charge of 1 coulomb?
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?
Answer the following in brief.
Explain the effect of dilution of the solution on conductivity.
Answer the following in brief.
What is a salt bridge?
Answer the following in brief.
Write electrode reactions for the electrolysis of aqueous NaCl.
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?
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`
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?
Derive the relationship between standard cell potential and equilibrium constant of cell reaction.
Answer the following in brief.
It is impossible to measure the potential of a single electrode. Comment.
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?
Answer the following in brief.
Write the electrode reactions and net cell reaction in NICAD battery.
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.
Answer the following:
Explain electrolysis of molten NaCl.
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.
Equilibrium constant of the reaction, \[\ce{2Cu^{\oplus}_{(aq)} -> Cu^{2\oplus}_{(aq)} + Cu_{(s)}}\] is 1.2 × 106. What is the standard potential of the cell in which the reaction takes place?
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.
Calculate emf of the cell at 25°C.
Zn(s) | Zn2+ (0.08 M) || Cr3+ (0.1 M) | Cr(s)
E°Zn = −076V, E°Cr = −0.74V.
What is a cell constant? What are its units? How is it determined experimentally?
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?
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?
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.
Answer the following:
What are anode and cathode for Leclanche' dry cell?
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).
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).
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"))`
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"))`
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 5: Electrochemistry
Balbharati solutions for Chemistry [English] 12 Standard HSC chapter 5 - Electrochemistry
Shaalaa.com has the Maharashtra State Board Mathematics Chemistry [English] 12 Standard HSC Maharashtra State Board solutions in a manner that help students grasp basic concepts better and faster. The detailed, step-by-step solutions will help you understand the concepts better and clarify any confusion. Balbharati solutions for Mathematics Chemistry [English] 12 Standard HSC Maharashtra State Board 5 (Electrochemistry) include all questions with answers and detailed explanations. This will clear students' doubts about questions and improve their application skills while preparing for board exams.
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Concepts covered in Chemistry [English] 12 Standard HSC 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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