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ELECTROCHEMISTRY AND CHEMICAL KINETICS
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ELECTROCHEMISTRY AND CHEMICAL KINETICS
Very Short Answer Questions
Q1. What is a galvanic cell or a voltaic cell? Give one example.
Q2. Write the chemical reaction used in the construction of the Daniel cell together with the half-cell reactions.
Q3. Name the two half-cell reactions that are taking place in the Daniel cell.
Q4. How is a galvanic cell represented on paper as per IUPAC convention? Give one example.
Q5. Write the cell reaction taking place in the cell $\ce{Cu(s)/Cu^{2+} (aq) // Ag+ (aq)/Ag(s)}$
Q6. What is standard hydrogen electrode?
Q7. Give a neat sketch of standard hydrogen electrode
Q8. What is Nernst equation? Write the equation for an electrode with electrode reaction$\ce{ M^{n+} (aq) + ne^-<=> M(s)}$
Q9. A negative $\ce{ E^{\circ}}$ indicates that the redox couple is reducing couple___________ than $\ce{ H^+/H2}$ couple. (powerful or weak)
Q10. A positive$\ce{ E^{\circ}}$ indicates that the redox couple is a weaker- than H/H, couple. (oxidising or reducing) couple
Q11. Write the Nernst equation for the$\ce{ EMF}$ of the cell $\ce{Ni(s)/Ni^{2+} (aq)// Ag^+ (aq)/Ag}$
Q12. Write the cell reaction for which $\ce{ E_cell \,=E_cell^{\circ} \,\,- \frac{RT}{ 2F} In \frac{[Mg]}{ [Ag]}}$
Q13. How is$\ce{ E^{\circ}}$cell related mathematically to the equilibrium constant Ke of the cell reaction?
Q14. How is Gibbs energy $\ce{(G)}$ related to the cell emf$\ce{ (E)}$ mathematically?
Q15. Define conductivity of a material. Give its SI units.
Q16. What is cell constant of a conductivity cell?
Q17. Define molar conductivity$ \wedge_m $and how is it related to conductivity (k)?
Q18. Give the mathematical equation which gives the variation of molar conductivity $ \wedge_m $ with the molarity (c) of the solution.
Q19. State Kohlrausch's law of independent migration of ions.
Q20. State Faraday's first law of electrolysis.
Q21. State Faraday's second law of electrolysis.
Q22. What are the products obtained at the platinum anode and the platinum cathode respectively in the electrolysis of fused or molten $\ce{NaCl}$?
Q23. Give the products obtained at the platinum electrodes (cathode and anode) when aqueous solution of$\ce{ K2SO4}$ is electrolysed.
Q24. Write the chemical equation corresponding to the oxidation of $\ce{ H2O(1)}$ at the platinum anode.
Q25. Give the chemical equation that represents the reduction of liquid water $\ce{ H2O(1)}$ at the platinum cathode.
Q26. What is a primary battery? Give one example.
Q27. Give one example for a secondary battery, Give the cell reaction.
Q28. Give the cell reaction of nickel- cadmium secondary battery.
Q29. What is a fuel cell? How is it different from a conventional galvanic cell?
Q30. Give the electrode reactions occurring at the anode and at the cathode in $\ce{H2 , O2}$ fuel cell.
Q31. What is metallic corrosion? Give one example.
Q32. Give the electro-chemical reaction that represents the corrosion or rusting of iron.
Q33. Short Answer Type Questions
Q34. What are galvanic cells? Explain the working of a galvanic cell with a neat sketch taking Daniel cell as example.
Q35. Give the construction and working of a standard hydrogen electrode with a neat diagram.
Q36. State and explain Nernst equation with the help of a metallic electrode and a non-metallic electrode.
Q37. Explain with a suitable example the relation between the Gibbs energy of chemical reaction (G) and the functioning of the electrochemical cell.
Q38. On what factors the electrical conductance of an aqueous solution of electrolyte depends?
Q39. How is molar conductivity of an aqueous electrolyte solution measured experimentally?
Q40. Explain the variation of molar conductivity with the change in the concentration of the electrolyte. Give reasons.
Q41. State and explain Kohlrausch's law of independent migration of ions.
Q42. What is electrolysis? Give Faraday's first law of electrolysis.
Q43. What are the products obtained at the cathode and the anode during the electrolysis of the following when platinum electrodes are used in the electrolysis (a) Molten $\ce{KCI}$ (b) Aq. $\ce{CuSO4}$ solution (c) Aq.$\ce{ K2SO4}$ solution
Q44. What are primary and secondary batteries? Give one example for each.
Q45. What are fuel cells? How are they different from galvanic cells? Give the construction of $\ce{H2 , O2}$ , fuel cell.
Q46. What is metallic corrosion? Explain it with respect to iron corrosion.
Q47. Define the speed or rate of a reaction.
Q48. Assuming that the volume of the system is constant, derive the expression for the average rate of the system$\ce{ R->P }$ in terms of R and P. (time 't' sec] [R=reactant, P=product ].
Q49. What are the units of rate of reaction?
Q50. Draw the graphs that relate the concentrations (C) of the reactants and the reaction times(t) and the concentrations of the products (C) and the reaction times(t) in chemical reactions.
Q51. Write the equation for the rate of the reaction $\ce{5Br (aq) + BrO^-_3 (aq) + 6H^+ (aq) -> 3Br2 (aq) + 3H2O (1)}$
Q52. What is rate law? Illustrate with an example.
Q53. Mention a reaction for which the exponents of concentration terms are not the same as their stoichiometric coefficients in the rate equation.
Q54. Define Order of a reaction. Illustrate your answer with an example.
Q55. What are elementary reactions?
Q56. What are complex reactions? Name one Complex reaction.
Q57. Give the units of rate constants for Zero, first order and second order reactions.
Q58. Define molecularity of a reaction. Illustrate with an example.
Q59. What is rate determining step in a complex reaction?
Q60. Give the mechanism for the decomposition reaction of $\ce{H2O2}$ in alkaline medium catalysed by $\ce{I^-}$ ions.
Q61. Write the equation relating [R], [R], and reaction time 't' for a zero order reaction. [R]=concentration of reactant at time t' and [R], initial concentration of reactant
Q62. Draw the graph that relates the concentration 'R', of the reactant and 't' the reaction time for a zero Order reaction.
Q63. Give two examples for zero Order reactions.
Q64. Write the integrated equation for a first order reaction in terms of [R], [R], and 't'.
Q65. Give two examples for gaseous first order reactions.
Q66. For the reaction$\ce{ A(g)-> B(g) + C(g)}$ write the integrated rate equation in terms of total pressure 'P' and the partial pressures$\ce{ P_A P_B P_C}$.
Q67. What is half-life of a reaction? Illustrate your answer with an example.
Q68. Write the equation relating the half-life (1%) of a reaction and the rate constant 'k' for first order reaction
Q69. Write the equation useful to calculate half-life (1½) values for zero and first order reactions.
Q70. What are pseudo first order reactions? Give one example.
Q71. Write the Arrhenius equation for the rate constant (k) of a reaction
Q72. By how many times the rate constant increases for a rise of reaction temperature by 10°C?
Q73. Explain the term 'activation energy' of a reaction with a suitable diagram.
Q74. Write the equation which relates the rate constants $\ce{k_1}$ and $\ce{k_2}$ at temperatures $\ce{T_1}$ and$\ce{ T_2}$ of a reaction.
Q75. What is collision frequency (2) of a reaction? How is rate related to it for the reaction$\ce{ A+B -> Products.}$
Q76. Draw the graphs between potential energy - reaction coordinates for catalysed and uncatalysed reactions.
Q77. What is the effect of temperature on the rate constant?
Q78. Give the electro-chemical reaction that represents the corrosion or rusting of iron.
Q1. Define average rate of a reaction. How is the rate of reaction expressed in terms of change in the concentration of reactants and products for the following reactions (1) $\ce{2HI_{(g)} ->H2 (g)+ I2 (g)}$ (2) $\ce{ Hg_{(l)} + Cl_{2 (g)}-> HgCl_{2 (s)}}$ (3)$\ce{ 5 Br^- (aq) + BrO3^- (aq) + 6H^+ (aq) -> 3Br2 (aq) + 3H2O_{(l)}}$
Q2. What is rate equation? How is it obtained? Write the rate equations for (i) $\ce{ 2NO(g) + O2 (g) -> 2NO2 (g)}$ (2) $\ce{CHCl3 + Cl2 -> CCI4 + HCI}$ (3)$\ce{ CH3COOC2H5 (l) + H2O (l) -> CH3COOH(aq) + C2H5OH(aq)}$
Q3. Define and explain the order of a reaction. How is it obtained experimentally?
Q4. What is molecularity of a reaction? How is it different from the 'order' of a reaction? Name one bimolecular and one trimolecular gaseous reactions.
Q5. Derive the integrated rate equation for a zero order reaction.
Q6. Derive an integrated rate equation for a first order reaction.
Q7. Derive an integrated rate equation in terms of total pressure (P) and the partial pressures $\ce{ P_A P_B P_C}$. for the gaseous reaction$\ce{ A(g)-> B(g) + C(g)}$.
Q8. What is half-life (t½) of a reaction? Derive the equations for the 'half-life' value of zero and first order reactions.
Q9. What is Arrhenius equation? Derive an equation which describes the effect of rise of temperature (1) on the rate constant (k) of a reaction.
Q10. Discuss the effect of catalyst on the kinetics of a chemical reaction with a suitable diagram.
Q11. Describe the salient features of the collision theory of reaction rates of bimolecular reactions.
Q12. Explain the terms (a) Activation energy (Ea) (b) Collision frequency (2) (c) Probability factor (P) with respect to Arrhenius equation.
Q13. What are galvanic cells? Explain the working of a galvanic cell with a neat sketch taking Daniel cell as example.
Q14. Give the construction and working of a standard hydrogen electrode with a neat diagram.
Q15. State and explain Nernst equation with the help of a metallic electrode and a non-metallic electrode.
Q16. Explain with a suitable example the relation between the Gibbs energy of chemical reaction (G) and the functioning of the electrochemical cell.
Q17. On what factors the electrical conductance of an aqueous solution of electrolyte depends?
Q18. How is molar conductivity of an aqueous electrolyte solution measured experimentally?
Q19. Explain the variation of molar conductivity with the change in the concentration of the electrolyte. Give reasons.
Q20. State and explain Kohlrausch's law of independent migration of ions.
Q21. What is electrolysis? Give Faraday's first law of electrolysis.
Q22. What are the products obtained at the cathode and the anode during the electrolysis of the following when platinum electrodes are used in the electrolysis (a) Molten $\ce{ KCl}$ (b) Aq. $\ce{ CuSO4}$ solution (c) Aq. $\ce{ K2SO4}$ solution
Q23. What are primary and secondary batteries? Give one example for each.
Q24. What are fuel cells? How are they different from galvanic cells? Give the construction of $\ce{ H2 ,\, O2}$ fuel cell.
Q25. What is metallic corrosion? Explain it with respect to iron corrosion.
Q1. What are electro chemical cells? How are they constructed? Explain the working of the different types of galvanic cells.
Q2. What is electrical conductance of a solution? How is it measured experimentally?
Q3. Give the applications of Kohlrausch's law of independent migration of fons.
Q4. Give the different types of batteries and explain the construction and working of each type of battery.
Q5. Explain the following terms with suitable examples. (a) average rate of a reaction (b) slow and fast reactions (c) order of a reaction (d) molecularity of a reaction (e) activation energy of a reaction
Q6. Give two examples for each of zero order and first order reactions. Write the equations for the rate of a reaction in terms of concentration changes of reactants and products for the following reactions.(1) $\ce{A(g)+B(g) -> C(g) + D (g)}$ (2)$\ce{ A(g) -> B(g) + C(g)}$ (3) $\ce{A(g)+B(g) -> C(g)}$
Q7. Discuss the effect of temperature on the rate of a reaction. Derive necessary equations in this context.
Q8. Give a detailed account of the collision theory of reaction rates of bimolecular gaseous reactions.
Q9. What are electro chemical cells? How are they constructed? Explain the working of the different types of galvanic cells.
Q10. What is electrical conductance of a solution? How is it measured experimentally?
Q11. Give the applications of Kohlrausch's law of independent migration of ions.
Q12. Give the different types of batteries and explain the construction and working of each type of battery.