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Bachelor’s Degree Programme (BSCG) – SOLUTIONS, PHASE EQUILIBRIUM, CONDUCTANCE, ELECTROCHEMISTRY & FUNCTIONAL GROUP ORGANIC CHEMISTRY-II Solved Assignment Answer | BCHCT 135 | 2021-2022

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Bachelor’s Degree Programme (BSCG) – SOLUTIONS, PHASE EQUILIBRIUM, CONDUCTANCE, ELECTROCHEMISTRY & FUNCTIONAL GROUP ORGANIC CHEMISTRY-II Solved Assignment Answer | BCHCT 135 | 2021-2022

Free BCHCT 135 Solved Assignment Answer | SOLUTIONS, PHASE EQUILIBRIUM, CONDUCTANCE, ELECTROCHEMISTRY & FUNCTIONAL GROUP ORGANIC CHEMISTRY-II | For July 2021 – June 2022

IGNOU BCHCT 135 Solved Assignment, This assignment is the curriculum of the BACHELOR’S OF SCIENCE (BSCG) program. For other courses, students check our website categories section to find their courses and assignments over there.

BCHCT-135 SOLUTIONS, PHASE EQUILIBRIUM, CONDUCTANCE, ELECTROCHEMISTRY & FUNCTIONAL GROUP ORGANIC CHEMISTRY-II Solved Assignment 2021-2022

IGNOU BCHCT-135 SOLUTIONS, PHASE EQUILIBRIUM, CONDUCTANCE, ELECTROCHEMISTRY & FUNCTIONAL GROUP ORGANIC CHEMISTRY-II assignment are 100 marks. There are two sections – A and B. Students have to answer all the questions. Download IGNOU BCHCT-135 Assignment free without any registration, Students can easily download the IGNOU assignment question paper from the official website of the university. They are not required to pay any fees or charges for this.

Title NameBCHCT-135 Solved Assignment 2021-2022 | SOLUTIONS, PHASE EQUILIBRIUM, CONDUCTANCE, ELECTROCHEMISTRY & FUNCTIONAL GROUP ORGANIC CHEMISTRY-II
UniversityIGNOU
Service TypeSolved Assignment (Soft Copy/Q&A form)
CourseBSCG
LanguageEnglish
SemesterSession: July 2021 – January 2022
Short NameBCHCT-135
Assignment CodeBCHCT-135/TMA/January 2022
ProductAssignment of BCHCT-135 | 2021-2022
Submission DateValid from 1st July 2021 to 30th June 2022
Assignment PdfDownload Now

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The answer of BCHCT-135 | SOLUTIONS, PHASE EQUILIBRIUM, CONDUCTANCE, ELECTROCHEMISTRY & FUNCTIONAL GROUP ORGANIC CHEMISTRY-II | Solved Assignment 2021-2022:

Note: Attempt all questions. The marks for each question are indicated against it.

Part – A

1. Draw and explain the vapor pressure curve of a solution showing a positive deviation from Raoult’s law.

2. Explain the process of steam distillation with the help of a suitable diagram

3. (a) State Nernst distribution law and write the expression for distribution constant.
(b) Differentiate between true and metastable equilibrium.

4. Define any five of the following terms :
(i) A component
(ii) Critical point
(iii) Molar conductivity
(iv) Transference number
(v) Standard hydrogen electrode
(vi) Electrolytic cells

5. (a) What are degrees of freedom? What is the maximum number of degrees of freedom possible for a one-component system?
(b) An aliphatic carboxylic acid reacts with alcohol and the following equilibrium is established.
RCOOH + R’CH2OH <=> RCOOCH2R’ + H2O
What is the number of constituents and the number of components in the system?

6. (a) “A four-phase equilibrium is not possible in a one-component system.” Justify the statement.
(b) Draw the phase diagram for sulphur system and label the sublimation and fusion curves for monoclinic sulphur on it.

7. (a) Differentiate between conductance and conductivity of an electrolytic solution.
(b) The resistance of a conductivity cell filled with an electrolytic solution is observed to be 180 Ω. If the resistance of 0.1M KCl solution taken in the same cell was found to be 72 Ω calculate the conductivity of the given solution.
(Given: The conductivity of 0.1 M KCl solution = 1.29 S m-1 ).

8. (a) What is ionic mobility? How is it related to transference numbers?
(b) The cell reaction for a galvanic cell is given below
Cu(s) + 2Ag+(aq) →Cu2+ (aq) + 2Ag(s)
(i) Write the half-cell reactions at the anode and the cathode
(ii) Calculate the value of cell emf under standard conditions; use data from Table 7.1
(iii) Will the reaction be spontaneous as written?

9. (a) Differentiate electrolyte concentration cell and electrode concentration cells.
(b) The cell reaction for a galvanic cell is given below
Cu(s) + 2Ag+(aq) →Cu2+ (aq) + 2Ag(s)
(i) Write the half-cell reactions at the anode and the cathode
(ii) Calculate the value of cell emf under standard conditions; use data from Table 7.1
(iii) Will the reaction be spontaneous as written?

10. (a) Calculate the time for which a current of 0.65 A be passed through molten magnesium chloride to get 5 g of magnesium. (Given: Mm(Mg) =24.25 g mol -1)
(b) Draw a labeled schematic graph of a conductometric titration between a weak acid and a strong base.

Part – B

11. Explain Fischer esterification of carboxylic acids giving its mechanism.

12. How would you prepare the following?
(i) Ethanoic anhydride using ketene
(ii) A tertiary alcohol starting from an ester

13. (a) What are lactams? Write the structures of  -butyrolactam and  -valerolactam and give their IUPAC names.
(b) Draw the enantiomers of N-methylethanamine.

14. Explain the nitrosation reaction of secondary and tertiary amines giving suitable reactions.

15. How can you prepare 1,3,5-tribromobenzene? Why it cannot be prepared by bromination of benzene ?

16. How will you synthesise valine using Gabriel phthalimide synthesis? Explain giving the sequence of reactions involved.

17. Discuss ninhydrin test giving the reactions involved.

18. Explain Edman degradation giving the reactions involved in it. Give the advantage of this method.

19. (a) Explain the formation of methyl glycoside of - and - D-glucose. Also give their structures.
(b) Write the reactions involved when  -D-glucose is treated with excess of acetic anhydride in the presence of pyridine.

20. (a) Differentiate between reducing and non-reducing sugars giving one example of each type.
(b) Write the reaction of formation of maltose from its monomers giving appropriate structures with proper labeling.

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